calculate the mass of KHP required to react with 20 mL of 0.05M NaOH
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A student titrates an unknown amount of potassium hydrogen phthalate $\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}\right.$, often abbreviated $\mathrm{KHP}$ ) with $20.46 \mathrm{~mL}$ of a $0.1000 \mathrm{M} \mathrm{NaOH}$ solution. KHP (molar mass $=204.22$ $\mathrm{g} / \mathrm{mol}$ ) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?
A student titrates an unknown amount of potassium hydrogen phthalate $\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4},$ often abbreviated KHP) with \right. $20.46 \mathrm{mL}$ of a $0.1000-M \mathrm{NaOH}$ solution. KHP (molar mass $=$ $204.22 \mathrm{g} / \mathrm{mol}$ ) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?
'A titration of KHP required 20.02 mL of 0.2987 M NaOH: What was the original mass of KHP in the analyte?'
Ma Ednelyn L.
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