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Questions tagged 'pH Calculation'

7 questions

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Anonymous

Feb 10, 2025

How much more acetic acid (pKa = 4.76) than acetate should be in solution to maintain a pH of 4.00?

I need assistance with a chemistry problem related to buffer solutions. Specifically, I am trying to determine how much more acetic acid (with a pKa of 4.76) is needed than acetate to maintain a pH of...

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Anonymous

Jan 18, 2025

What is the [H+] of a solution with a pH of 5.6?

What is the concentration of hydrogen ions, [H+], in a solution with a pH of 5.6? Please use a scientific calculator to determine your answer. (Points: 3) a) 5.0 × 10⁵ b) 8.3 × 10⁶ c) 2.5 × 10⁶ d) 7.7...

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Anonymous

Dec 13, 2024

Phosphate systems form essential buffers in organisms. Calculate the pH of a buffer made by dissolving 0.880 mol of NaOH in 0.475

Phosphate systems serve as essential buffers in living organisms. In this context, please calculate the pH of a buffer created by dissolving 0.880 moles of NaOH in 0.475 liters of a 1.00 M solution of...

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Clare Beer

Nov 27, 2024

Determine [OH] of solution?

I need assistance in determining the hydroxide ion concentration ([OH^-]) of a solution that is 0.120 M in carbonate ions ((CO_3^{2-})). Additionally, I would like to calculate the pH and pOH of this...

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Anonymous

Nov 23, 2024

Calculate the ph of a buffer that is 0.020 m hf and 0.040 m naf. the ka for hf is 3.5 × 10-4.

Calculate the pH of a buffer solution that contains 0.020 M HF and 0.040 M NaF. The dissociation constant (Ka) for HF is 3.5 × 10⁻⁴.

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Susanna Towne

Nov 21, 2024

1)Calculate [OH^-] for 1.8×10^−3 M Sr(OH)2.?

1) Calculate the concentration of hydroxide ions, [OH⁻], for a 1.8 × 10⁻³ M solution of Sr(OH)₂. 2) Calculate the pH for a 1.8 × 10⁻³ M solution of Sr(OH)₂. 3) Calculate the concentration of hydroxide...

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Anonymous

Oct 30, 2024

What is the [H+] in a solution with pOH of 0.253?

What is the concentration of hydrogen ions ([H^+]) in a solution with a pOH of 0.253? The following options are provided: A: (5.58 \times 10^{-15} \, \text{M}) B: (1.79 \times 10^{-14} \, \text{M}) C:...