Q1.
What will be the pH of 1.0 M ammonium formate solution, if Ka = 1 × 10–4 and Kb = 1 × 10–5?
Q2.
Which salt will not undergo hydrolysis?
Q3.
HCOO⁻ + H₂O ⇌ HCOOH + OH⁻
Degree of hydrolysis for above reaction is given by:
Q4.
The pH of aqueous solution of sodium acetate is:
Q5.
If pKb for CN⁻ at 25°C is 4.7. The pH of 0.5 M aqueous NaCN solution is:
Q6.
The highest pH value is of:
Q7.
pH of K₂S solution is:
Q8.
For anionic hydrolysis, pH is given by:
Q9.
Ionisation constant of a weak acid is 10⁻⁴. Find out equilibrium constant for the reaction of this weak acid with strong base.
Q10.
Hydroxyl ion concentration [OH⁻] in the case of sodium acetate can be expressed as (where Ka is dissociation constant of CH₃COOH and C is the concentration of sodium acetate):
Q11.
Consider:
(a) FeCl₃ in water - Basic
(b) NH₄Cl in water - Acidic
(c) Ammonium acetate in water - Acidic
(d) Na₂CO₃ in water - Basic
Which is/are not correctly matched?
Q12.
Which of the following salts undergoes hydrolysis in water?
Q13.
A salt 'X' is dissolved in water of pH = 7. The resulting solution becomes alkaline in nature. The salt is made up of:
Q14.
The solubility product of sparingly soluble uni-univalent salt (AB type) is defined as the product of ionic concentration in a:
Q15.
If solubility of salts M₂X, QY₂ and PZ₂ are equal, then the relation between their Ksp will be:
Q16.
The expression of solubility product of mercurous iodide is:
Q17.
At 25°C, the Ksp value of AgCl is 1.8 × 10⁻¹⁰. If 10⁻⁵ moles of Ag⁺ are added to solution then Ksp will be:
Q18.
At 25°C, the volume of water required to dissolve 1g BaSO₄ (Ksp = 1.0 × 10⁻¹⁰) will be (Molecular weight of BaSO₄ = 233):
Q19.
Concentration of Ag⁺ ions in saturated solution of Ag₂CrO₄ at 20°C is 1.5 × 10⁻⁴ mol L⁻¹. At 20°C, the solubility product of Ag₂CrO₄ is:
Q20.
If the concentration of CrO₄²⁻ ion in a saturated solution of silver chromate will be 2 × 10⁻⁴ M, solubility product of silver chromate will be:
Q21.
If the solubility of AgCl (formula mass=143) in water at 25°C is 1.43 × 10⁻⁴ g/100 mL of solution then the value of Ksp will be:
Q22.
The solubility product of As₂S₃ is given by the expression:
Q23.
If the solubility of PbBr₂ is 'S' g molecules per litre, considering 100% ionisation its solubility product is:
Q24.
If the solubility of lithium sodium hexafluoro aluminate Li₃Na₃(AlF₆)₂ is 'S' mol L⁻¹. Its solubility product is equal to:
Q25.
One litre of saturated solution of CaCO₃ is evaporated to dryness, when 7.0 g of residue is left. The solubility product for CaCO₃ is:
Q26.
Solubility of AgBr will be minimum in:
Q27.
In which of the following, the solution of AgSCN will be unsaturated:
Q28.
If 's' and 'S' are solubility and solubility product of a sparingly soluble binary electrolyte respectively then:
Q29.
The solubility product of CuS, Ag₂S and HgS are 10⁻³⁷, 10⁻⁴⁴ and 10⁻⁵⁴ respectively. The solubility of these sulphides will be in the order:
Q30.
If the maximum concentration of PbCl₂ in water is 0.01 M at 298 K, its maximum concentration in 0.1 M NaCl will be:
Q31.
M₂SO₄ (M⁺ is a monovalent metal ion) has a Ksp of 1.2 × 10⁻⁵ at 298 K. The maximum concentration of M⁺ ion that could be attained in a saturated solution of this solid at 298 K is:
Q32.
Which of the following has maximum solubility (Ksp value is given in brackets):
Q33.
Maximum soluble is (Ksp is given):
Q34.
In which of the following, the solubility of AgCl will be maximum:
Q35.
The solubility product of three sparingly soluble salts are given below:
1. PQ: 4.0 × 10⁻²⁰
2. PQ₂: 3.2 × 10⁻¹⁴
3. PQ₃: 2.7 × 10⁻³⁵
The correct order of decreasing molar solubility is:
Q36.
The Ksp value for Gd(OH)₃ is 2.8 × 10⁻²³. Find the pH of saturated solution of Gd(OH)₃:
Q37.
If the solubility product of AgBrO₃ and Ag₂SO₄ are 5.5 × 10⁻⁵ and 2 × 10⁻⁵ respectively, the relationship between their solubilities can be correctly represented as:
Q38.
Solubility product of Mg(OH)₂ is 1 × 10⁻¹¹. At what pH, precipitation of Mg(OH)₂ will begin from 0.1 M Mg²⁺ solution:
Q39.
A solution, containing 0.01 M Zn²⁺ and 0.01 M Cu²⁺ is saturated by passing H₂S gas. The S²⁻ concentration is 8.1 × 10⁻²¹ M, Ksp for ZnS and CuS are 3.0 × 10⁻²² and 8.0 × 10⁻³⁶ respectively. Which of the following will occur in the solution:
Q40.
What will happen if the pH of the solution of 0.001 M Mg(NO₃)₂ solution is adjusted to pH = 9 (Ksp Mg(OH)₂ = 8.9 × 10⁻¹²)
Q41.
The solubility product constant Ksp of Mg(OH)₂ is 9.0 × 10⁻¹². If a solution is 0.010 M with respect to Mg²⁺ ion, what is the maximum hydroxide ion concentration which could be present without causing the precipitation of Mg(OH)₂:
Q42.
When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because:
Q43.
Two monobasic weak acids have the same moles of H⁺ ions. What is the relationship between dissociation constant and dilution:
Q44.
Two solutions having same concentration of H⁺ ions are called:
Q45.
The pH of a formic acid which is 0.1% dissociated is equal to 4. What will be the pH of another weak monobasic acid (same concentration) which is 1% dissociated
Q46.
pH of water is 7. When any substance Y is dissolved in water then pH becomes 13. Substance Y is a salt of:
Q47.
Minimum pH is shown by aqueous solution of:
Q48.
Given:
(a) 0.005 M H₂SO₄
(b) 0.1 M Na₂SO₄
(c) 10⁻² M NaOH
(d) 0.01 M HCl
Choose the correct code having same pH:
Q49.
In the following solutions, the conc. of different acids are given, which mixture of the acid has highest pH:
Q50.
If 100 mL of pH = 3 and 400 mL of pH = 3 solutions are mixed, what will be the final pH of mixture
Q51.
10⁻⁶ M HCl is diluted 100 times. Its pH is:
Q52.
pH of 0.001M acetic acid would be:
Q53.
At 90°C, the pH of 0.001M KOH solution will be
Q54.
The pH of solution is increased from 3 to 6. Its H⁺ ion concentration will be:
Q55.
A solution has pOH equal to 13 at 298 K. The solution will be:
Q56.
The pH of the solution containing 10 mL of a 0.1M NaOH and 10 mL of 0.05M H₂SO₄ would be
Q57.
In a solution of pH = 5, more acid is added in order to reduce the pH upto 2. The increase in hydrogen ion concentration is:
Q58.
The hydrogen ion concentration in a given solution is 6 × 10⁻⁴ M. Its pH will be:
Q59.
The pOH of a solution is 10.0. The hydrogen ion concentration will be:
(a) 10⁻¹⁰ (b) Kw/10⁻¹⁰ (c) Kw/10⁻⁸ (d) 10⁻⁴
Select the correct combination:
Q60.
An aqueous solution whose pH = 0 is:
Q61.
Following five solutions of KOH were prepared as:
First: 0.1 moles in 1 L
Second: 0.2 moles in 2 L
Third: 0.3 moles in 3 L
Fourth: 0.4 moles in 4 L
Fifth: 0.5 moles in 5 L
The pH of resultant solution is:
Q62.
The pH of a 0.02 M ammonia solution which is 5% ionised will be:
Q63.
For N/10 H₂SO₄, pH value is:
Q64.
An aqueous solution of HCl is 10⁻⁹ M HCl. The pH of the solution should be:
Q65.
How many moles of HCl must be removed from 1 litre of aqueous HCl solution to change its pH from 2 to 3:
Q66.
8 g NaOH and 4.9 g H₂SO₄ are present in one litre of the solution. What is its pH
Q67.
Calculate pH of a solution whose 100 mL contains 0.2 g NaOH dissolved in it:
Q68.
What is the quantity of NaOH present in 250 cc of the solution, so that it gives a pH = 13:
Q69.
0.001 mol of the strong electrolyte M(OH)₂ has been dissolved to make a 20 mL of its saturated solution. Its pH will be: [K_w = 1 \times 10⁻¹⁴]
Q70.
Choose the wrong statement:
Q71.
The pH of 0.1 M solution of the following salts increases in order:
Q72.
In a buffer solution the ratio of concentration of NH₄Cl and NH₄OH is 1:1. When it changes to 2:1, pH of buffer:
Q73.
To 50 mL of 0.05M formic acid, how much volume of 0.10M sodium formate must be added to get a buffer solution of pH = 4.0? (pK_a of the acid is 3.8)
Q74.
In the volumetric estimation of HCl, if we make use of phenolphthalein as an indicator, which base is unsuitable for the titration:
Q75.
In a mixture of weak acid and its salt, the ratio of concentration of acid to salt is increased ten-fold. The pH of the solution:
Q76.
pK_b for NH₄OH at certain temperature is 4.74. The pH of basic buffer containing equimolar concentration of NH₄OH and NH₄Cl will be:
Q77.
What is the suitable indicator for titration of NaOH and oxalic acid:
Q78.
Phenolphthalein does not act as an indicator for the titration between:
Q79.
Which can act as buffer:
Q80.
The buffer solution play an important role in:
Q81.
K_a for HCN is 5 × 10⁻¹⁰ at 25°C. For maintaining a constant pH of 9, the volume of 5M KCN solution required to be added to 10mL of 2M HCN solution is:
Q82.
Buffering action of a mixture of CH₃COOH and CH₃COONa is maximum when the ratio of salt to acid is equal to:
Q83.
The pink colour of phenolphthalein in alkaline medium is due to:
Q84.
Which indicator works in the pH range 8 – 9.8
Q85.
A basic buffer will obey the equation pOH – pK_b = 1 only under condition:
Q86.
For weak acid-strong base titration, the indicator used is:
Q87.
For which of the following titration, methyl orange is a best indicator:
Q88.
The total number of different kind of buffers obtained during the titration of H₃PO₄ with NaOH are:
Q89.
A certain acidic buffer solution contains equal concentration of X⁻ and HX. The K_b for X⁻ is 10⁻¹⁰. The pH of the buffer is:
Q90.
When 1.0 mL of dil. HCl acid is added to 100 mL of a buffer solution of pH 4.0. The pH of the solution
Q91.
The pH of blood is maintained by CO₂ and H₂CO₃ in the body and chemical constituents of blood. This phenomenon is called:
Q92.
Phenolphthalein is not a good indicator for titrating
Q93.
Which of the following solutions does not act as buffer:
Q94.
On addition of NaOH to CH₃COOH solution, 60% of the acid is neutralised. If pK_a of CH₃COOH is 4.7 then the pH of the resulting solution is:
Q95.
500 mL of 0.2 M acetic acid are added to 500 mL of 0.30 M sodium acetate solution. If the dissociation constant of acetic acid is 1.5 × 10⁻⁵ then pH of the resulting solution is:
Q96.
Half of the formic acid solution is neutralised on addition of a KOH solution to it. If K_a (HCOOH) = 2 × 10⁻⁴ then pH of the solution is: (log 2 = 0.3010)
Q97.
A solution contains 0.2M NH₄OH and 0.2M NH₄Cl. If 1.0 mL of 0.001 M HCl is added to it. What will be the [OH⁻] of the resulting solution [K_b = 2 × 10⁻⁵]:
Q98.
Henderson equation pH – pK_a = 1 will be applicable to an acidic buffer when:
Q99.
0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution. What will be the OH⁻ ion concentration of this solution: K_b(NH₄OH) = 1.8 × 10⁻⁵
Q100.
When 0.02 moles of NaOH are added to a litre of buffer solution, its pH changes from 5.75 to 5.80. What is its buffer capacity:
Q101.
Calculate the pH of a buffer prepared by mixing 300 cc of 0.3 M NH₃ and 500 cc of 0.5 M NH₄Cl. K_b for NH₃ = 1.8 × 10⁻⁵:
Q102.
Calculate the ratio of pH of a solution containing 1 mole of CH₃COONa + 1 mole of HCl per litre and of other solution containing 1 mole CH₃COONa + 1 mole of acetic acid per litre:
Q103.
When 20 mL of M/20 NaOH are added to 10 mL of M/10 HCl, the resulting solution will:
Q104.
10 mL of a solution contains 0.1 M NH₄Cl + 0.01 M NH₄OH. Which addition would not change the pH of solution:
Q105.
N/10 acetic acid was titrated with N/10 NaOH. When 25%, 50% and 75% of titration is over then the pH of solution will be: [K_a = 10⁻⁵]
Q106.
The conjugate acid of O²⁻ is:
Q107.
Ionization constant of AOH and BOH base are K_b₁ and K_b₂. Their relation is pK_b₁ < pK_b₂. Conjugate of following base, does not show maximum pH:
Q108.
Select the species which can function as lewis base, bronsted acid and bronsted base:
(a) H₂O (b) NH₄⁺ (c) N³⁻
Correct code is:
Q109.
Which ion does not show acid behaviour:
Q110.
An example of Lewis acid is:
Q111.
In the reaction NH₃ + H₂O ⇌ NH₄⁺ + OH⁻ water behaves as:
Q112.
Which acts as Lewis base in the reaction BCl₃ + :PH₃ → Cl₃B←PH₃
Q113.
Which acts as Lewis acid in the reaction SnCl₂ + 2Cl⁻ → [SnCl₄]²⁻
Q114.
The conjugate base of (CH₃)₂NH₂⁺ is:
Q115.
Which equilibrium can be described as Lewis acid base reaction but not Bronsted acid base reaction:
Q116.
Conjugate base of hydrazoic acid is:
Q117.
NH₃ gas dissolves in water to give NH₄OH, in this reaction, water acts as:
Q118.
When ammonia is added to water, it decreases the concentration of which of the following ion
Q119.
The strongest acid among the following is
Q120.
Which of the following is not a Bronsted acid:
Q121.
Which of the following example behave as a Lewis acid BF₃, SnCl₂, SnCl₄:
Q122.
In the reaction HNO₃ + H₂O ⇌ H₃O⁺ + NO₃⁻, the conjugate base of HNO₃ is:
Q123.
The conjugate base of the weak acid in the reaction HBr + H₂O ⇌ H₃O⁺ + Br⁻ is
Q124.
In the reaction, AlCl₃ + Cl⁻ → [AlCl₄]⁻, AlCl₃ acts as:
Q125.
Mg²⁺ is _______ than Al³⁺:
Q126.
The two Bronsted bases in the reaction HC₂O₄⁻ + PO₄³⁻ ⇌ HPO₄²⁻ + C₂O₄²⁻ are
Q127.
The compound HCl behaves as ---- in the reaction, HCl + HF ⇌ H₂Cl⁺ + F⁻
Q128.
Which of the following is not a lewis base:
Q129.
Which of the following is Bronsted Lowry acid:
Q130.
The conjugate base for bicarbonate ion is:
Q131.
HCl does not behave as acid in:
Q132.
Which of the following is a base according to Bronsted-Lowry concept:
Q133.
In which of the following reactions NH₃ acts as acid
Q134.
According to Bronsted concept, the acids in the following reaction NH₃ + H₂O ⇌ NH₄⁺ + OH⁻ are:
Q136.
Which of the following is strongest conjugate base
Q137.
Which of the following species can act as Lewis base:
Q138.
A compound having the formula NH₂CH₂COOH may behave:
Q139.
Which of the following can act both as Bronsted acid and Bronsted base:
Q140.
The strongest conjugate base is:
Q141.
Aluminium chloride is:
Q144.
Species which do not act both as Bronsted acid and base is:
Q145.
Which one of the following is strong Lewis base & Bronsted acid & bronsted base:
Q146.
Which of the following is not a correct statement
Q147.
For the reaction NH₄⁺ + S²⁻ ⇌ NH₃ + HS⁻, NH₃ and S²⁻ are a group of:
Q148.
According to Arrhenius theory, acids are substances that dissociate in water to give ...(X) ... ions and bases are substances that produce ...(Y).... ions. Here, (X) and (Y) refer to
Q149.
"An acid is substance that is capable of donating a proton (H⁺) and base is a substance capable of accepting a proton (H⁺)." The above statement is justified by
Q150.
The concentration of [H⁺] and concentration of [OH⁻] of a 0.1 M aqueous solution of 2% ionised weak acid is [K_w = 1 × 10⁻¹⁴]:
Q151.
The solubility of BaSO₄ in water is 2.33 × 10⁻³ gL⁻¹. Its solubility product will be (molecular weight of BaSO₄ = 233):
Q152.
What will be the H⁺ ion concentration when 4 g NaOH dissolved in 1000 mL of water:
Q153.
When 10 mL of 0.1 M acetic acid (pK_a = 5.0) is titrated against 10 mL of 0.1 M ammonia solution (pK_b = 5.0), the equivalence point occurs at pH:
Q154.
At 25°C, the dissociation constant of a base BOH is 1.0 × 10⁻⁸. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:
Q155.
The solubility product of BaSO₄ at 25°C is 1.0 × 10⁻⁹. What would be the concentration of H₂SO₄ necessary to precipitate BaSO₄ from a solution of 0.01 M Ba²⁺ ions:
Q156.
pH of the solution of HCOONH₄ is 6.48. This can be explained by:
Q157.
The correct representation of solubility product of SnS₂ is:
Q158.
A solution of FeCl₃ in water acts as acidic due to:
Q159.
The pK_a of HNO₂ is 3.37. The pH of HNO₂ in its 0.01 mol L⁻¹ aqueous solution will be:
Q160.
When 0.01 M HCl is added in aqueous solution of acetic acid then:
Q161.
Solubility of MX₂ type electrolyte is 0.5 × 10⁻⁴ mol L⁻¹ then find out K_sp of electrolyte:
Q162.
A solution of MgCl₂ in water has pH:
Q163.
K_sp of Ca₃(PO₄)₂ is:
Q164.
An acid HA has dissociated in following manner HA ⇌ H⁺ + A⁻. It has concentration 1 M and pH = 5 then find out dissociation constant:
Q165.
Aqueous solution of Al₂(SO₄)₃ is:
Q166.
In a saturated solution of the sparingly soluble salt AgIO₃ (Molecular mass = 283). The equilibrium which sets in is AgIO₃(s) ⇌ Ag⁺(aq) + IO₃⁻(aq). If the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 × 10⁻⁸, what is the mass of AgIO₃ contained in 100 mL of its saturated solution:
Q167.
The solubility product of AgCl is 1 × 10⁻¹⁰, then molar solubility of AgCl is:
Q168.
K_a for CH₃COOH is 1.8 × 10⁻⁵. Find out the percentage dissociation of 0.2M CH₃COOH in 0.1M HCl solution
Q169.
The pK_a of a weak acid HA is 4.80. The pK_b of weak base BOH is 4.78. The pH of an aqueous solution of the corresponding salt BA will be:
Q170.
0.2M solution of HCOOH is 3.2% ionised then find ionisation constant of acid:
Q171.
Three reactions involving H₂PO₄⁻ are given below:
(i) H₃PO₄ + H₂O → H₃O⁺ + H₂PO₄⁻
(ii) H₂PO₄⁻ + H₂O → HPO₄²⁻ + H₃O⁺
(iii) H₂PO₄⁻ + OH⁻ → H₃PO₄ + O²⁻
In which of the above does H₂PO₄⁻ act as an acid?
Q172.
Given that for HA acid, K_a = 10⁻⁶ and for MOH base K_b = 10⁻⁶. The pH of 0.1 M MA salt solution will be:
Q173.
The K_sp for Cr(OH)₃ is 1.6 × 10⁻³⁰. The molar solubility of this compound in water is:
Q174.
An acid HA ionises as HA ⇌ H⁺ + A⁻. The pH of 1.0 M solution is 5. Its dissociation constant would be:
Q175.
The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, K_a of this acid is:
Q176.
What volume of 0.1M H₂SO₄ is needed to completely neutralize 40 mL of 0.2M NaOH solution:
Q177.
If pH value of a solution is 3 and on adding water, it becomes 6, then the dilution is increased by:
Q178.
In the reaction I₂ + I⁻ → I₃⁻, the Lewis base is:
Q179.
Which one of the following compounds is not a protonic acid:
Q180.
Which one of the following is NOT a buffer solution:
Q181.
The rapid change of pH near the end point of an acid–base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In⁻) forms of the indicator by the expression:
Q182.
The correct order of acidic strength is:
Q183.
Concentrations of NH₄Cl and NH₄OH in a buffer solution are in the ratio 1 : 10. If K_b for NH₄OH is 10⁻¹⁰, then pH of the buffer is:
Q184.
When HF is dissolved in formic acid, the equilibrium established is: HF + HCOOH ⇌ F⁻ + HCOOH₂⁺. The pair of species acting as [acid, conjugate acid] and [Base, conjugate base] respectively are:
Q185.
In a mixture of equimolar solutions of NaHCO₃ and NaOH, the species present in solution shall be:
Q186.
An aqueous solution contains [H⁺] = 10⁻⁴. If it is diluted by mixing equal volume of water then the concentration of OH⁻ in mol dm⁻³ will be:
Q187.
Which of the following is right for diprotic acid:
Q188.
The first and second dissociation constants of an acid H₂A are 1.0 × 10⁻⁵ and 5.0 × 10⁻¹⁰ respectively. The overall dissociation constant of the acid will be:
Q189.
50 mL solution of 0.1M CH₃COOH (pK_a = 4.73) is titrated with 0.1M NaOH solution, pH of solution when half of CH₃COOH is neutralized
Q190.
The pH of an aqueous solution of a 1 × 10⁻⁷ M solution of HCl will be:
Q191.
What will be the concentration of H⁺ ions in a solution containing 0.1M acetic acid and 0.1M sodium acetate if dissociation constant of acetic acid is 1.8 × 10⁻⁵:
Q192.
Which of the following pair constitutes a buffer:
Q193.
The hydrogen ion concentration of a 10⁻⁸ M HCl aqueous solution at 298 K (K_w = 10⁻¹⁴) is:
Q194.
Calculate the pOH of a solution at 25°C that contains 1×10⁻¹⁰M of hydronium ions, i.e., H₃O⁺
Q195.
A weak acid HA has a K_a of 1.00 × 10⁻⁵. If 0.100 moles of this acid is dissolved in one litre of water. The percentage of acid dissociated at equilibrium is closest to:
Q196.
Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest pH?
Q197.
Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture?
Q198.
NaCl exists in ...(X)... state as a cluster of positively charged sodium ions and negatively charged chloride ions which are held together due to ...(Y).... interactions between oppositely charged species. Here, (X) and (Y) refer to
Q199.
At 25°C, calculate the pH of 500 mL of aqueous solution containing 0.74 gm of Ca(OH)₂?
Q200.
Determine the volume of water required to dissolve 20mg of CaSO₄ at 298 K. (K_sp of CaSO₄ at 298K = 9 × 10⁻⁶)
Q201.
0.01 M NaX solution is 1% hydrolysed. Find the ionisation constant of weak acid HX and pH of NaX solution.
Q202.
Point out the conjugate acids for the following Bronsted bases NH₂⁻, NH₃ and HCOO⁻ respectively