Question

Determine the pH of each solution : a) 3.1 X 10 ^-2 M HI b). 0.116 M HClO4 c). a solution that is 5.6×10−2 M in HClO4 and 2.8×10−2 M in HCl d). a solution that is 1.85% HCl by mass (Assume a density of 1.01 g/mL for the solution.)

Answer #1

: a) 3.1 X 10 ^-2 M HI

pH = -log(H) = -log(3.1*10^-2) = 1.50863

b). 0.116 M HClO4

pH = -lG(H+) = -log(0.116) = 0.93554

c). a solution that is 5.6×10−2 M in HClO4 and 2.8×10−2 M in HCl

H+ = 5.6*10^-2 + 2.8*10^-2 = 0.084 M

pH = -log(H) = -log(0.084) = 1.07572

d). a solution that is 1.85% HCl by mass (Assume a density of 1.01 g/mL for the solution.)

assume

m = 100 g in total so

m = 1.85 g ar eHCl

mol = mass/MW = 1.85/36 = 0.05138 mol

mass of water = 100-1.85 = 98.15 g of water

assume D= 1 g /ml then V = 98.15 ml

threfore

M = mol/V = 0.05138/(98.15 /1000) = 0.52348

pH = -log(H) = -log(0.52348) = 0.28109

Determine the pH of each solution.
8.40×10−2 M HClO4
a solution that is 5.2×10−2 M in HClO4 and
4.7×10−2 Min HCl
a solution that is 1.06% HCl by mass (Assume a density of 1.01
g/mL for the solution.)

Determine the pH of each of the following solutions.
Part A:
8.23×10−2 M HClO4
Express your answer to three decimal places.
Part B:
A solution that is 4.8×10−2 M in HClO4 and
5.0×10−2 M in HCl
Express your answer to two decimal places.
Part C:
A solution that is 1.04% HCl by mass (Assume a density of 1.01
g/mL for the solution.)

find pH - answers and work please
2.6×10−2 M HI
Express your answer to two decimal places.
pH =
SubmitMy AnswersGive
Up
Part B
0.117 M HClO4
Express your answer to three decimal places.
pH =
SubmitMy AnswersGive
Up
Part C
a solution that is 5.2×10−2 M in HClO4 and
2.8×10−2 M in HCl
Express your answer to two decimal places.
pH =
SubmitMy AnswersGive
Up
Part D
a solution that is 1.90% HCl by mass (Assume a density of...

For each strong acid solutions, determine [H3O+],[OH−], and
pH.
1. 0.18 M HCL
2. 2.7×10−2 M HNO3
3. a solution that is 5.8×10−2 M in HBr and
2.3×10−2 M in HNO3
4. a solution that is 0.700% HNO3 by mass (Assume a density of
1.01 g/mL for the solution.)

Calculate the pH of each of the following strong acid
solutions.
(a) 0.000289 M HI
pH =
(b) 0.653 g of HClO4 in 16.0 L of solution
pH =
(c) 56.0 mL of 3.50 M HI diluted to 3.30 L
pH =
(d) a mixture formed by adding 81.0 mL of 0.00598 M HI to 37.0
mL of 0.000890 M HClO4
pH =

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

For each strong acid solutions, determine [H3O+],[OH−], and pH.
(So, there should be three answers for each question).
1. 0.22 M HCl
2. 1.8×10−2 M HNO3
3. a solution that is 6.1×10−2 M in HBr and
1.9×10−2 M in HNO3
4. a solution that is 0.755% HNO3 by mass (Assume a density of
1.01 g/mL for the solution.)

For each strong acid solution, determine [H3O+],[OH−] , and pH .
A solution that is 0.860% HNO3 by mass (Assume a density of 1.01
g/mL for the solution.)

Calculate the pH of each of the following strong acid
solutions.
a. 4.28×10−2 M HNO3.
b. 0.260 g of HClO3 in 2.40 L of solution.
c. 20.00 mL of 2.00 M HCl diluted to 0.490 L .
d. A mixture formed by adding 57.0 mL of 1.5×10−2 M HCl to 170
mL of 1.0×10−2 M HI.

Calculate the pH of each of the following strong acid
solutions.
(a) 0.00458 M HCl
pH =
(b) 0.643 g of HClO4 in 37.0 L of
solution
pH =
(c) 60.0 mL of 1.00 M HCl diluted to 4.10 L
pH =
(d) a mixture formed by adding 69.0 mL of 0.000760 M HCl to 46.0
mL of 0.00882 M HClO4
pH =

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 25 minutes ago

asked 37 minutes ago

asked 51 minutes ago

asked 57 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago