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

The mass of unknown acid needed is 0.230 grams

Explanation:

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

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:

The chemical reaction for the reaction of KHP and NaOH follows

By Stoichiometry of the reaction:

1 mole of NaOH reacts with 1 mole of KHP.

So, 0.0015 moles of NaOH will react with = of KHP

Moles of KHP = 0.0015 moles

Molar mass of KHP = 204.22 g/mol

Putting values in above equation, we get:

We are given:

Mass of unknown acid = 75 % of Mass of KHP

So, mass of unknown acid =

Hence, the mass of unknown acid needed is 0.230 grams

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.