Question

Part A

Determine the [OH−] of a solution that is 0.110 M in CO32−.

Express your answer using two significant figures.

Part B

Determine the pH of a solution that is 0.110 M in CO32−.

Express your answer to two decimal places.

Part C

Determine the pOH of a solution that is 0.110 M in CO32−.

Express your answer to two decimal places.

Please work out all algebra when using the quadratic equation, thanks!

Answer #1

**Part 1)**

CO_{3}^{2-}(aq) + H_{2}O(l)
HCO_{3}^{-}(aq)
+ OH^{-}(aq) K_{b} =
1.8 x 10^{-4}

HCO_{3}^{-}(aq) + H_{2}O(l)
H_{2}CO_{3}(aq)
+ OH^{-}(aq) K_{b} = 2.5 x
10^{-8}

Since the second kb is much smaller than the first, the hydroxide ions generated by the second equillibrium may be neglected.

In the first dissociation, we can see that the concentrations of
both HCO_{3}^{-}(aq) and OH^{-}(aq) ions
are the same

Therefore,

Kb =
[HCO_{3}^{-}][OH^{-}]/[CO_{3}^{2-}]

1.8 x 10^{-4} = [x][x]/[0.110]

(1.8 x 10^{-4})[0.110] = x^{2}

0.198 x 10^{-4} = x^{2}

x = 0.0044

**[OH ^{-}] = 0.0044 M**

**Part 2)**

pOH = - log [OH^{-}]

pOH = - log [0.0044] = 2.35

**pOH = 2.35**

**Part 3)**

We have,

pH + pOH = 14

Therefore,

pH = 14 - pOH

pH = 14.00 - 2.35 = 11.65

**pH = 11.65**

Problem 16.45
Part A
Calculate [OH−] for 1.0×10−3 M Sr(OH)2.
Express your answer using two significant figures.
[OH−] =
2.0×10−3
M
SubmitMy AnswersGive
Up
Correct
Part B
Calculate pH for 1.0×10−3 M Sr(OH)2.
Express your answer using two decimal places.
pH =
11.30
SubmitMy AnswersGive
Up
Correct
Part C
Calculate [OH−] for 2.500 g of LiOH in 220.0 mL of solution.
Express your answer using four significant figures.
[OH−] =
0.4745
M
SubmitMy AnswersGive
Up
Correct
Significant Figures Feedback: Your...

Calculate the pH of each solution.
Part A
[OH−] = 6.8×10−11 M
Express your answer using two decimal places.
Part B
[OH−] = 3.6×10−3 M
Express your answer using two decimal places.
Part C
[OH−] = 8.8×10−12 M
Express your answer using two decimal places.
Part D
[OH−] = 9.4×10−4 M
Express your answer using two decimal places.

For each strong acid solutions, determine [H3O+],[OH−],
and pH.
Please Answer all parts separately Will be very helpful
!!!
Part A
0.20 M HCl
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
[H3O+], [OH−] = ________________ M
Part B
Express your answer to two decimal places.
pH= _______________
Part C
1.6×10−2 M HNO3
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
[H3O+], [OH−] = ______________ M...

Part B
Calculate the pH of a 0.10 M solution of barium
hydroxide, Ba(OH)2.
Express your answer numerically using two decimal places.
ph=
Part C
Calculate the pH of a 0.10 M solution of NaOH.
Express your answer numerically using two decimal places.
ph=
Part D
Calculate the pH of a 0.10 M solution of hydrazine,
N2H4. Kb for hydrazine is 1.3×10−6.
Express your answer numerically using two decimal places.
ph=
Part E
Calculate the pH of a 0.10 M...

Part A
7.6×10−3 M HBr,
Express your answer using two decimal places.
pH =
Part B
1.39 g of HNO3 in 550 mL of solution,
Express your answer using three decimal places.
pH =
Part C
2.80 mL of 0.290 M HClO4 diluted to 55.0 mL ,
Express your answer using three decimal places.
pH =
Part D
A solution formed by mixing 14.0 mL of 0.110 M HBr with 20.0 mL
of 0.220 M HCl.
Express your answer using...

Part A Find the [OH−] of a 0.45 M aniline (C6H5NH2) solution.
(The value of Kb for aniline (C6H5NH2) is 3.9×10−10.) Express your
answer to two significant figures and include the appropriate
units. [OH−] = SubmitMy AnswersGive Up Part B Find the pH of a
0.45 M aniline (C6H5NH2) solution. Express your answer using two
decimal places.

Problem 16.45 part 2
Part E
Calculate [OH−] for 1.60 mL of 0.130 M NaOH diluted to 1.50 L
.
Express your answer using three significant figures.
[OH−] =
M
SubmitMy AnswersGive
Up
Part F
Calculate pH for 1.60 mL of 0.130 M NaOH diluted to 1.50 L .
Express your answer using three decimal places.
pH =
SubmitMy AnswersGive
Up
Part G
Calculate [OH−] for a solution formed by adding 4.70 mL of 0.150
M KOH to 20.0 mL...

Calculate the [H3O+] of the following polyprotic acid solution:
0.400 M H3PO4. Express your answer using two significant figures.
[H3O+] = .
Part B Calculate the pH of this solution. Express your answer
using one decimal place. pH =
Part C Calculate the [H3O+] and pH of the following polyprotic
acid solution: 0.370 M H2C2O4. Express your answer using two
significant figures. [H3O+] =
Part D Calculate the pH of this solution. Express your answer
using two decimal places.

Calculate the [OH−] of each aqueous solution with the following
[H3O+].
Part A
coffee, 1.0×10−5 M
Express your answer using two significant figures.
[OH−] =
M
Part B
soap, 1.0×10−8 M
Express your answer using two significant figures.
[OH−] =
M
Part C
cleanser, 4.9×10−10 M
Express your answer using two significant figures.
[OH−] =
M
Part D
lemon juice, 2.5×10−2 M
Express your answer using two significant figures.
[OH−] =
M

Part A
[H3O+] = 2.1×10−4 M
Express your answer using two significant figures.
[OH−] = M
Part B
A.)
This solution is acidic.
B.)
This solution is basic.
C.)
This solution is neutral.

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