A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO₄ solution. Calculate the pH after the following volumes of acid have been added: (a) 20.0 mL. (b) 23.0 mL.

A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (c) 24.0 mL.

A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO₄ solution. Calculate the pH after the following volumes of acid have been added: (d) 25.0 mL. (e) 30.0 mL.

A 35.0-mL sample of 0.150 M acetic acid 1CH3COOH2 is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (b) 17.5 mL.

Consider the titration of 30.0 mL of 0.050 M NH₃ with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (b) 20.0 mL (c) 59.0 mL.

Consider the titration of 30.0 mL of 0.050 M NH₃ with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (e) 61.0 mL (f) 65.0 mL.

Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) sodium hydroxide (NaOH).

Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (b) hydroxylamine 1NH2OH2.

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr).

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (b) chlorous acid (HClO₂).

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (c) benzoic acid (C₆H₅COOH).

The solubility of two slightly soluble salts of M2 + , MA and MZ2, is the same, 4 * 10-4 mol/L. (c) If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+?

(a) True or false: 'solubility' and 'solubility-product constant' are the same number for a given compound.

(b) Write the expression for the solubility-product constant for each of the following ionic compounds: MnCO₃, Hg(OH)₂, and Cu₃(PO₄)₃.

(a) I f t he molar solubility of CaF₂ at 35°C i s 1.24 × 10^–3 mol/L, what is K_sp at this temperature?

(b) It is found that 1.1 × 10^-2 g SrF₂ dissolves per 100 mL of aqueous solution at 25°C. Calculate the solubility product for SrF₂.

(b) If 0.0490 g of AgIO₃ dissolves per liter of solution, calculate the solubility-product constant.

A 1.00-L solution saturated at 25 C with calcium oxalate 1CaC2O42 contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 C.

A 1.00-L solution saturated at 25 C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25 C.

Calculate the solubility of LaF3 in grams per liter in (a) pure water.

Calculate the solubility of LaF₃ in grams per liter in (b) 0.010 M KF solution.

Calculate the solubility of LaF₃ in grams per liter in (c) 0.050 M LaCl₃ solution.

Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF21s2. Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF2 at the bottom of the beaker increase, decrease, or remain the same?

Calculate the solubility of Mn(OH)₂ in grams per liter when buffered at pH (a) 7.0 (b) 9.5 (c) 11.8.

Calculate the molar solubility of Ni(OH)₂ when buffered at pH (a) 8.0.

Calculate the molar solubility of Ni(OH)₂ when buffered at pH (b) 10.0.

Calculate the molar solubility of Ni(OH)₂ when buffered at pH (c) 12.0.