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expeople1 [14]
3 years ago
12

After doing multiple titrations, your NaOH solution is determined to have a mean concentration value of 0.100 M. Given you are t

o assume your unknown acid is 75.0% KHP, how many grams of your unknown will you need to use 15.00 mL of your 0.100 M standardized NaOH
Chemistry
1 answer:
Mrac [35]3 years ago
7 0

<u>Answer:</u> The mass of unknown acid needed is 0.230 grams

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

Molarity of NaOH solution = 0.100 M

Volume of solution = 15.00 mL = 0.015 L    (Conversion factor:  1 L = 1000 mL)

Putting values in above equation, we get:

0.100M=\frac{\text{Moles of NaOH}}{0.015L}\\\\\text{Moles of NaOH}=(0.100mol/L\times 0.015L)=0.0015mol

The chemical reaction for the reaction of KHP and NaOH follows

KHC_8H_4O_4(aq.)+NaOH\rightarrow KNaC_8H_4O_4(aq.)+H_2O(l)

By Stoichiometry of the reaction:

1 mole of NaOH reacts with 1 mole of KHP.

So, 0.0015 moles of NaOH will react with = \frac{1}{1}\times 0.0015=0.0015mol of KHP

  • To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of KHP = 0.0015 moles

Molar mass of KHP = 204.22 g/mol

Putting values in above equation, we get:

0.0015mol=\frac{\text{Mass of KHP}}{204.22g/mol}\\\\\text{Mass of KHP}=(0.0015mol\times 204.22g/mol)=0.306g

We are given:

Mass of unknown acid = 75 % of Mass of KHP

So, mass of unknown acid = \frac{75}{100}\times 0.306=0.230g

Hence, the mass of unknown acid needed is 0.230 grams

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