The pH of a 0.77M solution of boric acid H3BO3 is measured to be
4.68. Calculate...
The pH of a 0.77M solution of boric acid H3BO3 is measured to be
4.68. Calculate the acid dissociation constant Ka of boric acid. Be
sure your answer has the correct number of significant digits.
Solutions
Expert Solution
Boric acids unlike other acids don't give away hydronium ion in
an aqueous solution, rather it helps water to produce hydronium ion
by taking OH- from water molecule.
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A) If a 10.0 mL solution of "acid rain" is measured to have a pH
of 2.75, what is the molar concentration of strong acid HNO3
formed? Hint: pH=-log[H+] and 10^-pH=[H+] is in molarity units.
B) The total acid concentration (nitric + nitrous acid) of the
10.0 mL solution of "acid rain" is determined by an acid-base
titration method. You add 5.00 mL of the titrant sodium hydroxide
with a concentration of 0.0114 M to reach the endpoint.
i. What...
Calculate the conjugate base to acid ratio in the solution.
Calculate the theoretical pH. Solution: 10.00 ml of .2M acetic acid
and 1.00 mL of .1 M sodium hydroxide and 9.00 mL distilled
water
Calculate the pH of a 0.67M oxalic acid solution and calculate
the pKb of the resulting ionic base that will form. (Look up Ka of
Oxalic acid)
Please show all work as I would like to learn how to do the
problem and not just have the answer. Thank you.
The pH of a 0.17-M solution of
maleic acid
(H2C4H2O4)
is measured to be 1.40. Use this information to
determine a value of Ka for maleic
acid.
H2C4H2O4(aq)
+ H2O(l) ((double arrow))
HC4H2O4-(aq)
+ H3O+(aq) Ka =
Calculate the pH of a solution that is 0.145 M in a propanol
acid (CH3CH2COOH) and 0.127 M in potassium propanoate (KCH3CH2COO).
The Ka of propanoic acid is 1.34x10^-5. Your answer should be
reported in three significant figures.
a) For 50mL of a 0.400M borate buffer at pH 8.5 (boric acid Ka =
5.8x10^-10), Describe how you would make this using sodium borate
(NaH2BO3) and 2.50M HCl.
b) what is the solution pH after adding 0.100 mL of concentrated
HCl to a 20.0 mL portion of this buffer?
c) What is the solution pH after adding 10.0 mL of 6.00 M NaOH
to a 20.0 mL portion of this original buffer?
Calculate the pH of each solution.
A. A solution containing 0.0133 M maleic acid and 0.0189 M
disodium maleate. The Ka values for maleic acid are 1.20×10−2 (Ka1)
and 5.37×10−7 (Ka2).
B. A solution containing 0.0368 M succinic acid and 0.022 M
potassium hydrogen succinate. The Ka values for succinic acid are
6.21×10−5 (Ka1) and 2.31×10−6 (Ka2).