Calculate the pH of each of the following strong acid
solutions.
(a) 0.00526 M HCl
pH =
(b) 0.839 g of HBr in 29.0 L of solution
pH =
(c) 46.0 mL of 8.80 M HCl diluted to 4.20 L
pH =
(d) a mixture formed by adding 76.0 mL of 0.00851 M HCl to 23.0 mL
of 0.00876 M HBr
pH =
Calculate the pH of each of the following strong acid
solutions.
(a) 0.00593 M HIO4
pH = ____
(b) 0.670 g of HCl in 50.0 L of solution
pH = ____
(c) 75.0 mL of 1.00 M HIO4 diluted to 2.30 L
pH = ____
(d) a mixture formed by adding 83.0 mL of 0.00358 M HIO4
to 30.0 mL of 0.000920 M HCl
pH = ____
Calculate the pH of each of the following strong acid
solutions.
(a) 0.00512 M HBr
pH =
(b) 0.633 g of HI in 18.0 L of solution
pH =
(c) 44.0 mL of 3.90 M HBr diluted to 1.30 L
pH =
(d) a mixture formed by adding 89.0 mL of 0.00215 M HBr to 89.0 mL
of 0.000310 M HI
pH =
Calculate [OH -] and pH for each of the following
solutions.
(a) 0.0034 M RbOH
[OH-] =_________ M
pH = _________
(b) 0.0872 g of KOH in 510.0 mL of solution
[OH -] =__________ M
pH = __________
(c) 79.8 mL of 0.00719 M Sr(OH)2 diluted to 900
mL
[OH -] = __________ M
pH = ____________
(d) A solution formed by mixing 64.0 mL of 0.000880 M
Sr(OH)2 with 36.0 mL of 2.6 x 10-3 M
RbOH
[OH -]...
Calculate [OH -] and pH for each of the following
solutions.
(a) 0.0043 M KOH
[OH-] = _____ M
pH = 11.63
(b) 0.0341 g of CsOH in 540.0 mL of solution
[OH -] = 4.21e-4 M
pH = 10.62
(c) 28.1 mL of 0.00187 M Ca(OH)2 diluted to 800
mL
[OH -] = _____ M
pH = 10.12
(d) A solution formed by mixing 71.0 mL of 0.000480 M
Ca(OH)2 with 24.0 mL of 1.3 x 10-3 M
KOH
[OH -] =...
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.170 M HClO(aq) with 0.170 M KOH(aq). The ionization constant for HClO can be found here.
(a) before addition of any KOH ______
(b) after addition of 25.0 mL of KOH _____
(c) after addition of 40.0 mL of KOH ______
(d) after addition of 50.0 mL of KOH ______
(e) after addition of 60.0 mL of KOH ______
Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.140 M pyridine, C5H5N(aq) with 0.140 M HBr(aq):
(a) before addition of any HBr
(b) after addition of 12.5 mL of HBr
(c) after addition of 20.0 mL of HBr
(d) after addition of 25.0 mL of HBr
(e) after addition of 37.0 mL of HBr
Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic
acid, CH3CO2H, is 1.8 × 10-5. If someone could list the steps and
calculations that would be helpful. Thank you!
Calculate the pH at the equivalence point in titrating 0.120
M solutions of each of the following with
9.0×10−2M NaOH.
A) hydrobromic acid (HBr)
B) chlorous acid (HClO2)
C) benzoic acid (C6H5COOH)