Question

Calculate the pH of solutions with the following concentrations.

A: [H3O+] = 1×10⁻¹² M

Express your answer using one decimal place

B: [OH−] = 1×10⁻⁵ M

Express your answer using one decimal place.

C;

3.00×10⁻³ mol of HBr are dissolved in water to make 16.0 L of solution. What is the concentration of hydroxide ions, [OH−], in this solution?

Express your answer with the appropriate units.

D:

8.00 g of NaOH are dissolved in water to make 4.00 L of solution. What is the concentration of hydronium ions, [H3O+], in this solution?

Express your answer with the appropriate units.

E:

A solution has [H3O+] = 8.0×10⁻⁶ M . Use the ion product constant of water

Kw=[H3O+][OH−]

to find the [OH−] of the solution.

Express your answer to two significant figures.

F:

A solution has [OH−] = 1.3×10⁻² M . Use the ion product constant of water

Kw=[H3O+][OH−]

to find the [H3O+] of the solution.

Express your answer to two significant figures

Answer 1

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