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4 years ago

What is the ph of the solution in which the h+ is 1.0 x10-4 mol/l

1 answer:

6 0

The definition and formula to calculate pH is:

pH = log { 1 / [H+] }

So, the pH of this solution, whose molar concentration of H+ is [H+] = 1.0 * 10^-4, is:

pH = log { 1 / (1.0 * 10 ^-4) } = log (10^4) = 4

Answer: option C. 4.00

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How many L of 3.0 M H2SO4 solution can be prepared by using 100.0 mL OF 18 M H2SO4?

max2010maxim [7]

Answer: A volume of 600 mL of 3.0 M $H_{2}SO_{4}$ solution can be prepared by using 100.0 mL OF 18 M $H_{2}SO_{4}$ .

Explanation:

Given: $V_{1}$ = ?, $M_{1} = 3.0 M\\$

$V_{2} = 100.0 mL$ , $M_{2} = 18 M$

Formula used to calculate the volume is as follows.

$M_{1}V_{1} = M_{2}V_{2}$

Substitute the values into above formula as follows.

$M_{1}V_{1} = M_{2}V_{2}\\3.0 M \times V_{1} = 18 M \times 100.0 mL\\V_{1} = \frac{18 M \times 100.0 mL}{3.0M}\\= 600 mL$

Thus, we can conclude that a volume of 600 mL of 3.0 M $H_{2}SO_{4}$ solution can be prepared by using 100.0 mL OF 18 M $H_{2}SO_{4}$ .

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3 years ago

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Ber [7]

Is there an image with this question

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3 years ago

Question 6 I need help

avanturin [10]

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3 years ago

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3 years ago

A can of butane with a pressure of 2 atm at 283k has its pressure increased to a new pressure of 5 atm. What is the temperature

Ber [7]

Answer:

New temperature T2 = 707.5 K (Approx.)

Explanation:

Given:

Old pressure P1 = 2 atm

Old temperature T1 = 283 K

New Pressure P2 = 5 atm

Find:

New temperature T2

Computation:

Using Gay-Lussac law;

P1 / T1 = P2 / T2

So,

2 / 283 = 5 / T2

New temperature T2 = 707.5 K (Approx.)

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3 years ago