Question

Calculate the pH of a solution with [H_{3}O+] = 1.0 x
10^{-8} M

please explain

Answer #1

Given [H_{3}O^{+}] = 1.010 ^{-8}
M

We know that pH = -log [H_{3}O^{+}]

= -log(1.010 ^{-8}
)

= -[log1.0+ log 10 ^{-8}
)
Since Log AB = log A + Log B

= - log 1.0 -(-8log 10
)
Since log A^{x} = x log A

= 0 + (8x1)

= 8

which is abuse since pH of an acidic solution should not exceeds 7

Sine the [H_{3}O^{+}] concentration is very
weak

Total But the [H_{3}O^{+}]_{total} =
[H_{3}O^{+}] _{from the acid} +
[H_{3}O^{+}] _{from water}

= 1.010 ^{-8}
M + 1.010 ^{-7}
M

= 1.010 ^{-7}
(0.1+1)

= 1.1 10 ^{-7}
M

So pH = -log [H_{3}O^{+}]_{total}

=
-log(1.110 ^{-7}
)

= -[log1.1+ log
10 ^{-7} )

= - log 1.1 +7 log 10

= -0.04 + 7

= 6.96

three sig figs please.
a) 0.19 M HCl
calculate [H3O+] , [OH-], and pH
b)1.5 x 10^ -2 M HNO3
calculate [H3O+] , [OH-], and pH
c) a solution that is 7.5×10−2 M in HBr and
1.9×10−2 M in HNO3
calculate [H3O+] , [OH-], and pH
d) a solution that is 0.780% HNO3
by mass (Assume a density of 1.01 g/mL for the
solution.)
calculate [H3O+] , [OH-], and pH

A. What is the pH of the following solutions?
i. [H3O+] = 1.0 X 10-6
ii. [H3O+] = 4.4 X 10-2
B. What volume in mL of 0.115 M sodium hydroxide would
neutralize 25.0 mL of a 0.106 M sulfuric acid solution during a
titration?

Calculate the ph of each solution given the following (H3O.+) or
(OH-) values
Part A- (H3O+ ) = 2.5 x10-8 M
Use TWO decimal places
Ph=_______
Part B- (H3O+) = 6.0 x 10-6M
Use TWO decimal places
Part C- (OH-) = 4.0 x 10-2 M
Use TWO decimal places
Part D - (OH-) = 7.5 x 10-3 M
Use TWO decimal places

Calculate the [H3O+] of the following polyprotic acid solution:
0.310 M H3PO4 Calculate the pH of this solution Calculate the
[H3O+] and pH of the following polyprotic acid solution: 0.360 M
H2C2O4. Calculate the pH of this solution.

Calculate the pH of each solution given the following [H3O+] or
[OH−] values.
Part A: [H3O+] = 3×10−4 M
Express your answer using one decimal place.
Part B: [H3O+] = 2×10−9 M
Part C: [OH−] = 4×10−5 M
Part D: [OH−] = 4.5×10−11 M
Part E: [H3O+] = 5.1×10−8 M
Part F: [OH−] = 8.0×10−4 M

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

What is the pH of a solution of
3.4 M H2A (Ka1 = 1.0 × 10^-6 and Ka2 is 1.0 × 10^-10)?
Please explain step by step

What is the H3O+ ion concentration in a 0.10 M solution of
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For each calculations calculate the pH of the solution and the
number of moles.
a) [H3O+]= 1.1(10^-3)M; V= 245 mL
b) [H3O+]= 6.0(10^-11)M; V= 105 mL

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