Q1.
Aqueous solution of which of the following compounds is the best conductor of electric current?
Q2.
Aqueous solution of acetic acid contains:
Q3.
Conjugate base for Bronsted acids H2O and HF are:
Q4.
Which of the following cannot act both as Bronsted acid and as Bronsted base?
Q5.
Which of the following fluoro-compounds is most likely to behave as a Lewis base?
Q6.
Which of these is least likely to act as a Lewis base?
Q7.
Which is the strongest acid in the following?
Q8.
Which one of the following molecular hydrides acts as a Lewis acid?
Q9.
Which of the following molecules acts as a Lewis acid?
Q10.
Which one of the following statements is not true?
Q11.
Which one of the following compounds is not a protonic acid?
Q12.
In HS–, I–, R – NH2, NH3 order of proton accepting tendency will be:
Q13.
Conjugate acid of NH2– is:
Q14.
Which compound is electron deficient?
Q15.
The strongest conjugate base is:
Q16.
Which of the following is not a Lewis acid?
Q17.
Repeated use of which one of the following fertilizers would increase the acidity of the soil?
Q18.
Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 × 10–15.
Q19.
The pH of 0.01 M NaOH(aq) solution will be:
Q20.
Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations. pH of which one of them will be equal to 1?
A. 60 mL M/10 HCl + 40 mL M/10 NaOH
B. 55 mL M/10 HCl + 45 mL M/10 NaOH
C. 75 mL M/5 HCl + 25 mL M/5 NaOH
D. 100 mL M/10 HCl + 100 mL M/10 NaOH
Q21.
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5N+H) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10–9) is:
Q22.
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Q23.
Which of the following salts will give highest pH in water?
Q24.
Accumulation of lactic acid (HC3H5O3), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociated. The value of dissociation constant, Ka, for this acid will be:
Karnataka NEET 2013
medium
Q25.
At 100°C the Kw of water is 55 times its value at 25°C. What will be the pH of neutral solution? (log 55 = 1.74)
Q26.
Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?
Q27.
What is [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.10 M in CH3COOH? (Ka for CH3COOH = 1.8 × 10–5)
Q28.
The ionization constant of ammonium hydroxide is 1.77 × 10–5 at 298 K. Hydrolysis constant of ammonium chloride is:
Q29.
What is the [OH–] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)2?
Q30.
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?
Q31.
A weak acid, HA, has a Ka of 1.00 × 10–5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to:
Q32.
Calculate the pOH of a solution at 25°C that contains 1 × 10–10 M of hydronium ions, i.e. H3O+.
Q33.
The hydrogen ion concentration of a 10–8 M HCl aqueous solution at 298 K (Kw = 10–14) is:
Q34.
At 25°C, the dissociation constant of a base, BOH, is 1.0 × 10–12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be:
Q35.
Which has highest pH?
Q36.
Ionisation constant of CH3COOH is 1.7 × 10–5 and concentration of H+ ions is 3.4 × 10–4. Then find out initial concentration of CH3COOH molecules.
Q37.
Correct relation between dissociation constants of a dibasic acid is:
Q38.
Which statement is wrong about pH and H+?
Q39.
The concentration of [H+] and concentration of [OH–] of a 0.1 aqueous solution of 2% ionised weak acid is [ionic product of water = 1 × 10–14]:
Q40.
The hydride ion H– is stronger base than its hydroxide ion OH–. Which of the following reaction will occur if sodium hydride (NaH) is dissolved in water?
Q41.
The ionic product of water at 25°C is 10–14. Its ionic product at 90°C will be:
Q42.
If α is dissociation constant, then the total number of moles for the reaction, 2HI → H2 + I2 will be:
Q43.
The pH value of N/10 NaOH solution is:
Q44.
The pH value of a 10 M solution of HCl is:
Q45.
At 80°C, distilled water has [H3O+] concentration equal to 1 × 10–6 mole/litre. The value of Kw at this temperature will be:
Q46.
0.1 M solution of which one of these substances will act basic?
Q47.
The compound whose water solution has the highest pH is:
Q48.
Which will make basic buffer?
Q49.
Which one of the following pairs of solutions is not an acidic buffer?
Q50.
The dissociation constant of a weak acid is 1 × 10–4. In order to prepare a buffer solution with a pH = 5, the [Salt]/[Acid] ratio should be:
Q51.
Buffer solutions have constant acidity and alkalinity because:
Q52.
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution? (log 2.7 = 0.43)
Q53.
In a buffer solution containing equal concentration of B– and HB, the Kb for B– is 10–10. The pH of buffer solution is:
Q54.
Which of the following pairs constitutes a buffer?
Q55.
The rapid change of pH near the stoichiometric 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:
Q56.
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. Then find out pKb of NH4OH.
Q57.
A physician wishes to prepare a buffer solution at pH = 3.85 that efficiently resists changes in pH yet contains only small concentration of the buffering agents. Which of the following weak acids together with its sodium salt would be best to use?
Q58.
The pH value of blood does not appreciably change by a small addition of an acid or a base, because the blood:
Q59.
pH of a saturated solution of Ca(OH)2 is 9. The solubility product (Ksp) of Ca(OH)2 is:
Q60.
The molar solubility of CaF2 (Ksp = 5.3 × 10–11) in 0.1 M solution of NaF will be:
Q61.
The solubility of BaSO4 in water is 2.42 × 10–3 g L–1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO4 = 233 g mol–1):
Q62.
Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.2 × 10–4 mol L–1. Solubility product of Ag2C2O4 is:
Q63.
The solubility of AgCl(s) with solubility product 1.6 × 10–10 in 0.1 M NaCl solution would be:
Q64.
MY and NY3, two nearly insoluble salts, have the same Ksp values of 6.2 × 10–13 at room temperature. Which statement would be true in regard to MY and NY3?
Q65.
The Ksp of Ag2CrO4, AgCl, AgBr and AgI are respectively, 1.1 × 10–12, 1.8 × 10–10, 5.0 × 10–13, 8.3 × 10–17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, NaI and Na2CrO4?
Q66.
Using the Gibbs' energy change, ΔG° = +63.3 kJ, for the following reaction, Ag2CO3(s) ⇌ 2Ag+(aq) + CO32–(aq), the Ksp of Ag2CO3(s) in water at 25°C is (R = 8.314 J K–1 mol–1):
Q67.
The values of Ksp of CaCO3 and CaC2O4 are 4.7 × 10–9 and 1.3 × 10–9 respectively at 25°C. If the mixture of these two is washed with water, what is the concentration of Ca2+ ions in water?
Q68.
Identify the correct order of solubility in aqueous medium:
Q69.
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is:
Q70.
In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and Pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl– concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium? (Ksp for AgCl = 1.8 × 10–10, Ksp for PbCl2 = 1.7 × 10–5):
Q71.
H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because:
Q72.
The solubility product of a sparingly soluble salt AX2 is 3.2 × 10–11. Its solubility (in moles/L) is:
Q73.
The solubility product of AgI at 25°C is 1.0 × 10–16 mol2 L–2. The solubility of AgI in 10–4 N solution of KI at 25°C is approximately (in mol L–1):
Q74.
Solubility of MX2 type electrolytes is 0.5 × 10–4 mol/lit., then find out Ksp of electrolytes.
Q75.
Solubility of M2S salt is 3.5 × 10–6 then find out solubility product.
Q76.
The solubility of a saturated solution of calcium fluoride is 2 × 10–4 moles per litre. Its solubility product is:
Q77.
The solubility product of CuS, Ag2S and HgS are 10–31, 10–44 and 10–54 respectively. The solubilities of these sulphides are in the order:
Q78.
The solubility of AgCl will be minimum in:
Q79.
Which one of the following is most soluble?
Q80.
Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 × 10–15.
Q81.
Which among the following salt solutions is basic in nature?
NEET (UG) 2020 (COVID-19)
easy
Q82.
The solubility product for a salt of the type AB is 4 × 10–8. What is the molarity of its standard solution?
NEET (UG) 2020 (COVID-19)
medium
Q83.
The pKb of dimethylamine and pKa of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethylammonium acetate solution is:
Q84.
Silver iodide is used in cloud seeding to produce rain AgI(s) ⇌ Ag+(aq) + I–(aq); Ksp = 8.5 × 10–7. AgNO3 and KI are mixed to give [Ag+] = 0.010 M; [I–] = 0.015 M. Will AgI precipitate?
NEET(UG) 2021 (Paper-2)
medium
Q85.
100 ml of a mixture of NaOH and Na2SO4 is neutralised by 10 ml of 0.5 M H2SO4. Hence NaOH in 100 ml solution is:
NEET(UG) 2021 (Paper-2)
medium
Q86.
200 mL of 0.1 M H3BO3 solution on complete neutralisation requires ....... mL of 0.5 M NaOH solution.
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medium
Q87.
The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is [Given pKa of CH3COOH = 4.57]
Q88.
The solubility product of BaSO4 in water is 1.5 × 10–9. The molar solubility of BaSO4 in 0.1 M solution of Ba(NO3)2 is:
NEET (UG) 2022 (OVERSEAS)
medium
Q89.
0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is:
Q90.
For a weak acid HA, the percentage of dissociation is nearly 1% at equilibrium. If the concentration of acid is 0.1 mol L⁻¹, then the correct option for its Ka at the same temperature will be:
Q91.
Which combination of the following substances will result in the formation of an acidic buffer when mixed? (Given: pKa of the acid = pKb of the base)
Q92.
Amongst the given options, which of the following molecules/ions acts as a Lewis acid?
Q93.
The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is: (Given: Solubility product of AgCl = 10⁻¹⁰)