Answer:
0.5050g of KHP were titrated
Explanation:
<em>... (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?</em>
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The KHP is a salt used as standard to determine concentrations of bases as NaOH solutions. The reaction that occurs is:
KHP + NaOH → KP⁻Na⁺ + H₂O
<em>Only 1 hydrogen is acidic. Only 1 hydrogen reacts with NaOH</em>
In the reaction you can see that 1 mole of NaOH reacts per mole of KHP
To find mass of KHP we need to determine its moles finding moles of NaOH (The moles of KHP required to reach endpoint = Moles of NaOH added):
<em>Moles NaOH:</em>
21.30mL = 0.02130L * (0.1161mol / L) = 0.002473 moles of NaOH = Moles KPH
With mass of KHP and its molar mass we can solve the mass of KHP:
0.002473 moles of KHP * (204.22g/mol) =
<h3>0.5050g of KHP were titrated</h3>
