1) Part A What is the H+ concentration for an aqueous solution with pOH = 3.04 a

Question

1)

Part A

What is the H+ concentration for an aqueous solution with pOH = 3.04 at 25 C?

Express your answer to two significant figures and include the appropriate units.

Part B

Arrange the following aqueous solutions, all at 25 C, in order of decreasing acidity.

Rank from most acidic to most basic. To rank items as equivalent, overlap them.

pH= 5.45 , 0.0023 M HCl, 0.0018 KOH, pOH= 8.55

Most acidic ?

Most Basic ?

Part C

At a certain temperature, the pH of a neutral solution is 7.29. What is the value of Kw at that temperature?

Express your answer numerically using two significant figures.

2)

Calculate [H3O+] in each aqueous solution at 25C, and classify each solution as acidic or basic.

A

[OH]= 5.2×104 M

Express your answer using two significant figures.

B

[OH]= 1.4×1012 M

Express your answer using two significant figures.

3)

Part A

0.50 g of hydrogen chloride (HCl) is dissolved in water to make 8.0 L  of solution. What is the pH of the resulting hydrochloric acid solution?

Express the pH numerically to two decimal places.

Part B

0.60 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 7.5 L of solution. What is the pH of this solution?

Express the pH numerically to two decimal places.

4)

Part A

What assumption is commonly used to simplify the process of finding the pH for a solution of a weak acid?

What assumption is commonly used to simplify the process of finding the pH for a solution of a weak acid?

The concentration of H3O+ is assumed to be directly found from the K a expression, so all that is needed is to plug the initial concentrations of each species into the K a expression.

5)

A certain weak acid, HA, has a Ka value of 8.9×107.

Part A

Calculate the percent ionization of HA in a 0.10 M solution.

Express your answer to two significant figures and include the appropriate units.

Part B

Calculate the percent ionization of HA in a 0.010 M solution.

Express your answer to two significant figures, and include the appropriate units.

6)

What mass of HClO4 should be present in 0.600 L of solution to obtain a solution with each pH?

pH = 1.40

Express your answer using two significant figures.

7)

Part A

Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 1.2×105.

Express your answer to two decimal places.

Part B

Find the percent ionization of a 0.130 M solution of a weak monoprotic acid having Ka= 1.2×105.

Express your answer using two significant figures.

The concentration of H3O+ in solution is assumed to be equal to the concentration of the weak acid. For many weak acid solutions, it is assumed that [H3O+] is small relative to the initial concentration of acid, so the "x is small" approximation is used. The quadratic equation is the fastest way to find the pH of a weak acid, and the assumption is that the quadratic equation will work.

The concentration of H3O+ is assumed to be directly found from the K a expression, so all that is needed is to plug the initial concentrations of each species into the K a expression.

5)

A certain weak acid, HA, has a Ka value of 8.9×107.

Part A

Calculate the percent ionization of HA in a 0.10 M solution.

Express your answer to two significant figures and include the appropriate units.

Part B

Calculate the percent ionization of HA in a 0.010 M solution.

Express your answer to two significant figures, and include the appropriate units.

6)

What mass of HClO4 should be present in 0.600 L of solution to obtain a solution with each pH?

pH = 1.40

Express your answer using two significant figures.

7)

Part A

Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 1.2×105.

Express your answer to two decimal places.

Part B

Find the percent ionization of a 0.130 M solution of a weak monoprotic acid having Ka= 1.2×105.

Express your answer using two significant figures.

Explanation / Answer

1)

Part A

What is the H+ concentration for an aqueous solution with pOH = 3.04 at 25 C?

Express your answer to two significant figures and include the appropriate units.

pH = 14-pOH

pH = 14-3.04 = 10.96

[H+] = 10^-10.96 = 1.09*10^-11

[H] =  1.09*10^-11

Part B

Arrange the following aqueous solutions, all at 25 C, in order of decreasing acidity.

Rank from most acidic to most basic. To rank items as equivalent, overlap them.

pH= 5.45 , 0.0023 M HCl, 0.0018 KOH, pOH= 8.55

Most acidic = HCl

Most Basic = KOH

NOTE:

please consider posting multiple questions in multiple sets of the Q&A. We are not allowed to answer multiple questions

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