Calculate the pH after 0.017 mole of HCl is added to 1.00 L of each of the four solutions. (Assume that all solutions are at 25°C.)

(a) 0.133 *M* acetic acid (HC_{2}H_{3}O_{2}, *K*_{a} = 1.8 **✕** 10^{−5})

(b) 0.133 *M* sodium acetate (NaC_{2}H_{3}O_{2})

(c) pure H_{2}O

(d) 0.133 *M* HC_{2}H_{3}O_{2} and 0.133 *M* NaC_{2}H_{3}O_{2}

Consider a solution that contains both C_{6}H_{5}NH_{2} and C_{6}H_{5}NH_{3}^{+}. Calculate the ratio [C_{6}H_{5}NH_{2}]/[C_{6}H_{5}NH_{3}^{+}] if the solution has the following pH values. (Assume that the solution is at 25°C.)

(a) pH = 5.16

(b) pH = 5.53

(c) pH = 4.74

(d) pH = 4.93

Consider the titration of 41.5 mL of 0.198 *M* HCl with 0.124 *M* NaOH. Calculate the pH of the resulting solution after the following volumes of NaOH have been added. (Assume that all solutions are at 25°C.)

(a) 0.0 mL

(b) 10.0 mL

(c) 40.0 mL

(d) 80.0 mL

(e) 100.0 mL

Consider the titration of 100.0 mL of 0.240 *M* benzoic acid (*K*_{a} = 6.4 **✕** 10^{−5}) with 0.120 *M* KOH. Calculate the pH of the resulting solution after each of the following volumes of KOH has been added. (Assume that all solutions are at 25°C.)

(a) 0.0 mL

(b) 50.0 mL

(c) 100.0 mL

(d) 150.0 mL

(e) 200.0 mL

(f) 250.0 mL

Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (Assume that the temperature is 25°C.)

(a) 101.1 mL of 0.17 *M* HF (*K*_{a}= 7.2 **✕** 10^{−4}) titrated with 0.17 *M* KOH

halfway point | |

equivalence point |

(b) 100.7 mL of 0.15 *M* C_{2}H_{5}NH_{2} (*K*_{b} = 5.6 **✕** 10^{−4}) titrated with 0.30 *M* HNO_{3}

halfway point | |

equivalence point |

(c) 100.9 mL of 0.51 *M* HCl titrated with 0.26 *M* KOH

halfway point | |

equivalence point |

Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties.

(a) Ca_{3}(PO_{4})_{2}, *K*_{sp} = 1.3 **✕** 10^{−32}

mol/L

(b) MgF_{2}, *K*_{sp} = 6.4 **✕** 10^{−9}

mol/L

(c) AgBr, *K*_{sp} = 5.0 **✕** 10^{−13}

mol/L

The *K*_{sp} for silver chromate (Ag_{2}CrO_{4}) is 9.0 **✕** 10^{−12}. Calculate the solubility of silver chromate in each of the following.

(a) water

mol/L

(b) 0.15 *M* AgNO_{3}

mol/L

(c) 0.34 *M* Na_{2}CrO_{4}

mol/L

Use the following data to calculate the *K*_{sp} value for each solid.

(a) The solubility of MnCO_{3} is 1.1 **✕** 10^{−3} g/L.

(b) The solubility of Al(OH)_{3} is 5.5 **✕** 10^{−9} mol/L.

The concentration of Ba^{2+} in a solution saturated with BaF_{2}(*s*) is 1.82 **✕** 10^{−2} *M*. Calculate *K*_{sp} for BaF_{2}.

Calculate the solubility (in mol/L) of Co(OH)_{3} (*K*_{sp} = 3 **✕** 10^{−43}) in each of the following. (Assume that all solutions are at 25°C.)

(a) water (assume pH is 7.0 and constant)

mol/L

(b) a solution buffered at pH = 5.5

mol/L

(c) a solution buffered at pH = 10.9

mol/L