a)
[H+]left = 0.075 - 0.072 = 3 x 10^-3 M
pH = -log [H+]
pH = 2.52
b)
pKa = 8.60
HBrO + NaOH -----------------> NaBrO + H2O
0.075 0.072 0 0
3 x 10^-3 0.072
pH = pKa + log [NaBrO / HBrO]
pH = 8.60 + log (0.072 / 3 x 10^-3)
pH = 9.98
c)
pKa = 4.20
C6H5COOH + NaOH -----------------> C6H5COO- + H2O
0.075 0.072 0 0
3 x 10^-3 0.072
pH = 4.20 + log (0.072 / 3 x 10^-3)
pH = 5.58
39. + -10.1 points 0/4 Submissions Used Calculate the pH at the equivalence point in titrating...
Calculate the pH at the equivalence point in titrating 0.047 M
solutions of each of the following with 0.055 M NaOH.
(a) nitric acid (HNO3)
pH =
(b) acetic acid (HC2H3O2),
Ka = 1.8e-05
pH =
(c) benzoic acid (HC7H5O2),
Ka = 6.3e-05
pH =
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H302), Ka = 1.84-05...
Calculate the pH at the equivalence point in titrating 0.028 M solutions of each of the following with 0.031 M NaOH. (a) nitric acid (HNO3) pH = ______ (b) benzoic acid (HC7H5O2), Ka = 6.3e-05 pH = _______ (c) hypobromous acid (HBrO), Ka = 2.5e-09 pH = _______
Calculate the pH at the equivalence point in titrating 0.047 M
solutions of each of the following with 0.055 M NaOH.
(a) nitric acid (HNO3)
pH =
(b) acetic acid (HC2H3O2),
Ka = 1.8e-05
pH =
(c) benzoic acid (HC7H5O2),
Ka = 6.3e-05
pH =
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH (a) nitric acid (HNO3) pH= (b) аcetic acid (HC2H302), ка = 1.8e-05 pH =...
7.48 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), (b) chlorous acid (HCIO2)
26. + -/0.1 points 0/4 Submissions Used A buffer solution contains 0.45 mol of benzoic acid (HC7H502) and 0.33 mol of sodium benzoate (NaCzH502) in 3.70 L. The Ka of benzoic acid (HC7H502) is Ka = 6.30-05. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.31 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the...
Calculate the pH at the equivalence point in titrating 0.056 M solutions of each of the following with 0.013 M NaOH. (a) nitric acid (HNO3) pH = (b) arsenous acid (H3AsO3), Ka = 5.1e-10 pH = (c) ascorbic acid (HC6H7O6), Ka = 8e-05 pH =
22. + -10.1 points 0/4 Submissions Used Determine the pH of each of the following solutions. (a) 0.360 M phenol (weak acid with Ka = 1.3e-10). (b) 0.458 M hydrogen peroxide (weak acid with Ka = 2.4e-12). (c) 0.238 M pyridine (weak base with Kb = 1.7e-09).
Calculate the pH at the equivalence point in titrating 0.051 M solutions of each of the following with 0.051 M NaOH. (a) perbromic acid (HBrO4) pH = (b) carbonic acid (H2CO3), Ka = 4.3e-07 pH = (c) boric acid (H3BO3), Ka = 5.8e-10 pH =
Calculate the pH at the equivalence point in titrating 0.063 M solutions of each of the following with 0.083 M NaOH. (a) perchloric acid (HCIO 4) pH = 7 (b) hydrocyanic acid (HCN), k, = 4.9e-10 pH = (c) boric acid (H3B03), ka = 5.8e-10 pH =
21. + -10.1 points 0/4 Submissions Used Calculate the pH of each of the following strong acid solutions. (a) 0.00373 M HBr pH = (b) 0.319 g of HBrO4 in 10.0 L of solution pH = (C) 11.0 mL of 8.30 M HBr diluted to 2.00 L pH = (d) a mixture formed by adding 61.0 mL of 0.00320 M HBr to 50.0 mL of 0.00888 M HBrO4 pH =