4. pH of a saturated solution of Ca(OH) 2 is 9. The Solubility product (

. pH of a saturated solution of Ca(OH) is . The Solubility product ( sp K of Ca(OH) a) . - b) .

- c) . - d) . - . Conjugate base for Bronsted acids H O and HF are a) OH and H FH , respectively b) H O and F , respectively c) OH and F , respectively d) H O and H F , respectively .

Which will make basic buffer? a) mL of .1M NaOH+25mL of .1M CH COOH b) mL of .1M CH COOH+ mL of .1M NH OH c) mL of .1M HCl+ mL of .1M NH OH d) mL of .1M HCl+ mL of .1M NaOH EVALUATION . Which of the following fluro compounds is most likely to behave as a Lewis base? (NEET – ) a) BF b) PF c) CF d) SiF .

Which of these is not likely to act as Lewis base? a) BF b) PF c) CO d) F – . The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively a) acidic, acidic, basic b) basic, acidic, basic c) basic, neutral, basic d) none of these . The percentage of pyridine (C H N) that forms pyridinium ion (C H NH) in a .10M aqueous pyridine solution - b (K for C H N= .

% . Equal volumes of three acid solutions of pH , and are mixed in a vessel. What will be the H + ion concentration in the mixture? a) .

- b) - c) . d) none of these . The solubility of AgCl (s) with solubility product . - in .1M NaCl solution would be a) .

M - b) . M - c) . M - d) Zero . If the solubility product of lead iodide is .

- , its solubility will be a) - × M b) M - c) . M - d) . M - . MY and NY , are insoluble salts and have the same K sp values of .

- at room temperature. Which statement would be true with regard to MY and NY ? a) The salts MY and NY are more soluble in .5M KY than in pure water b) The addition of the salt of KY to the suspension of MY and NY will have no effect on their solubility’s c) The molar solubilities of MY and NY in water are identical d) The molar solubility of MY in water is less than that of NY . What is the pH of the resulting solution when equal volumes of .1M NaOH and .01M HCl are mixed?

The dissociation constant of a weak acid is - . In order to prepare a buffer solution with a pH = , the [Acid] [Salt] ratio should be a) : b) : c) : d) . The pH of M KOH - solution will be a) b) c) d) none of these . H PO - the conjugate base of a) PO − b) P O c) H PO d) HPO - .

Which of the following can act as Lowry – Bronsted acid as well as base? a) HCl b) SO − c) HPO − d) Br . The pH of an aqueous solution is Zero. The solution is a) slightly acidic b) strongly acidic c) neutral d) basic .

The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by a) [H ]= K [acid] [salt] a b) [H ]= K [salt] a c) [H ]=K [acid] a d) [H ]= K [salt] [acid] a . Which of the following relation is correct for degree of hydrolysis of ammonium acetate? a) h = K h b) h = K K a b c) w a b K h = K .K d) h = K .K K a b w . Dissociation constant of NH OH is .

- the hydrolysis constant of NH Cl would be a) . - b) - . c) . - d) .

- Answer the following questions: . What are Lewis acids and bases? Give two example for each. .

Discuss the Lowry – Bronsted concept of acids and bases. . Indentify the conjugate acid base pair for the following reaction in aqueous solution i)HS (aq) + HF F (aq) + H S(aq) ii) HPO + SO -  - - - PO + HSO iii)NH + CO NH + HCO   . Account for the acidic nature of HClO in terms of Bronsted – Lowry theory, identify its conjugate base.

. When aqueous ammonia is added to CuSO solution, the solution turns deep blue due to the formation of tetramminecopper (II) complex, [Cu(H O) ] +4NH (aq) [Cu(NH ) ] (aq) + (aq) +  , among H O and NH Which is stronger Lewis base. . The concentration of hydroxide ion in a water sample is found to be .

M - . Identify the nature of the solution. . A lab assistant prepared a solution by adding a calculated quantity of HCl gas at C o to get a solution with [H O ]= M - .

Is the solution neutral (or) acidic (or) basic. . Calculate the pH of . M HNO Solution.

. Define solubility product . Define ionic product of water. Give its value at room temperature.

. Explain common ion effect with an example . Derive an expression for Ostwald’s dilution law . Define pH .

Calculate the pH of - . × M solution of Ba (OH) . 50ml of .05M HNO is added to 50ml of .025M KOH . Calculate the pH of the resultant solution.

. The K a value for HCN is - . What is the pH of .4M HCN solution? .

Calculate the extent of hydrolysis and the pH of . M ammonium acetate Given that K =K = . a b - . Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base .

Solubility product of Ag CrO is - . What is the solubility of Ag CrO in .01M AgNO solution? . Write the expression for the solubility product of Ca (PO ) .

A saturated solution, prepared by dissolving CaF (s) in water, has [Ca ]= . M + - What is the K sp of CaF ? . K sp of AgCl is .

× − . Calculate molar solubility in M AgNO . A particular saturated solution of silver chromate Ag CrO has [Ag ]= - and [CrO ] = . M.

- What is the value of K sp for Ag CrO ? . Write the expression for the solubility product of Hg Cl . .

K sp of Ag CrO is . - . what is solubility of Ag CrO in .1M K CrO . .

Will a precipitate be formed when . L of .1M Pb(NO ) and .100L of . M NaCl are mixed? K (PbCl )= .

. sp - . K sp of Al(OH) is M - . At what pH does .

M Al - + precipitate on the addition of buffer of NH Cl and NH OH solution? Buffers and pH Step – Open the Browser and type the URL given (or) Scan the QR Code. You can see a webpage as shown in the figure. Step – Now you can select a combination of an acid/base (Box ) and its corresponding salt (Box ) from the given choices and also select the desired concentrations (Box ) and volume (Box ) of these for the buffer.

Step – In order to measure the pH of the made-up buffer click the ‘Insert Probe’ (Box ) on the pH meter. Now the pH meter shows the pH. After measuring you need to remove the probe by clicking ‘Remove Probe” (Box ) to make any changes in the composition. Step – Now you can vary the concentration and volume of the components and see how the pH changes.

By using this tool you can simulate the preparation of a buffer and measure its pH values Please go to the URL tgreenbo/pHbuffer20.html (or) Scan the QR code on the right side