Table of contents

3. Chemical Reactions

Stoichiometry

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Multiple Choice

What is the expected mass of KHP (potassium hydrogen phthalate) required to react completely with 44.32 mL of KOH solution if the molarity of KOH is 0.566 M?

5.00 g

1.25 g

3.75 g

2.50 g

Verified step by step guidance

First, understand the chemical reaction between KHP (potassium hydrogen phthalate) and KOH. The balanced equation is:

{K HP}_{1} (aq) + {K OH}_{1} (aq) \to {K KP}_{1} (aq) + {H 2 O}_{1} (l)

. This shows a 1:1 molar ratio between KHP and KOH.

Calculate the moles of KOH using the formula:

moles = molarity \times volume

. Convert the volume from mL to L by dividing by 1000:

44.32 \times 0.001 = 0.04432

Substitute the values into the moles formula:

moles = 0.566 \times 0.04432

. This will give you the moles of KOH, which is equal to the moles of KHP needed due to the 1:1 ratio.

Determine the molar mass of KHP. The chemical formula for KHP is

{K HC 8 H 4 O 4}_{1}

. Calculate the molar mass by adding the atomic masses of each element: K (39.10 g/mol), H (1.01 g/mol), C (12.01 g/mol), O (16.00 g/mol).

Finally, calculate the mass of KHP required using the formula:

mass = moles \times molar mass

. Substitute the moles of KHP and the molar mass of KHP into this formula to find the expected mass.

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