Problem1:calculate the ph of each of the following solution:
(A)0.0010 M HCl
(B)0.76 M KOH
Problem2:calculate the hydrogen ion concentration in mol ⁄ L for solutions with the following pH values:
(A)2.42
(B)11.21
(C)6.96
(D)15.00
Problem3:How much NaOH (in grams) is needed to prepare 546 mL of solution with a pH of10.00 ?
Problem4:calculate the pH of 1.00 L of the buffer 1.00 M CH3COONa ⁄ 1.00 M CH3COOH before and the addition of :
(A)0.080 mol NaOH
(B)0.12 mol HCl
Assumethat there is no change in volume.
Problem5: A solution mad eby mixing 5.00 × 102 mL of 0.167 MNaOH with 5.00 × 102 mL of 0.100 M CH3COOH. Calculate theequilibrium concentrations of H+, CH3COOH, CH3COO-,OH- and Na +
Problem 6: Balance the following redoxequations using half reaction method:
(A) H2O2 + Fe2+Fe3+ + H2O
(B) Cu- + HNO3Cu2++NO + H2O
( C ) CN- + MnO4-CNO-+MnO2
(D) Br2BrO3 – +Br-
(E) S2O32-+ I2I-+ S4O62-
Problem 7: predict whether the following reaction would occurspontaneously in aqueous solution at 25 C. Assume that the initialconcentrations of dissolved species are all 1.0 M
(A) Mg (s) + Pb2+(aq) Mg2+(aq) + Pb(s)
(B) Br2 (I) + 2I- (aq) 2Br-(aq) +I2(s)
(C ) O2(g) + 4H+(aq)+4Fe2+ (aq) 2H2O(I) + 4Fe3+(aq)
(D) 2Al(s) +3I2(s) 2Al3+(aq) +6I- (aq)
Problem 8: which spcies in each pairis a better reducing agent under standard state conditions?
(A)Na or Li
(B) H2 or l2
(C ) Fe2+ or Ag
(D) Br- or Co2+