Ca(KC8H4O4)2(aq) + 2 H2O(l) What Is The Number Of Grams Of KHP ...

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A student determined the percent of potassium hydrogen phthalate (KHC8H4O4), commonly abbreviated as KHP, in an impure sample of KHP. A 6.450 g sample of impure KHP required 32.50 mL of 0.275 M calcium hydroxide, Ca(OH)2, solution for titration. The molar mass of KHP is 204.2 g/mol. Calcium hydroxide reacts with KHP, as shown in Equation: 2 KHC8H4O4(aq) + Ca(OH)2(aq) -> Ca(KC8H4O4)2(aq) + 2 H2O(l). What is the number of grams of KHP present in the impure KHP sample? A student determined the percent of potassium hydrogen phthalate (KHC8H4O4), commonly abbreviated as KHP, in an impure sample of KHP. A 6.450 g sample of impure KHP required 32.50 mL of 0.275 M calcium hydroxide, Ca(OH)2, solution for titration. The molar mass of KHP is 204.2 g/mol. Calcium hydroxide reacts with KHP, as shown in Equation: 2 KHC8H4O4(aq) + Ca(OH)2(aq) -> Ca(KC8H4O4)2(aq) + 2 H2O(l). What is the number of grams of KHP present in the impure KHP sample? Show more…

Added by James M.

Step 1

First, we need to find the moles of Ca(OH)2 used in the titration. We can do this using the formula: moles = Molarity × Volume (in Liters) moles of Ca(OH)2 = 0.275 M × 0.0325 L = 0.0089375 mol Show more…

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A student titrates an unknown amount of potassium hydrogen phthalate (KHC8H4O4, often abbreviated KHP) with 20.67 mL of a 0.1400 M solution. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution? Mass = ? g?

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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?

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A student titrates an unknown amount of potassium hydrogen phthalate $\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}, \text { often abbreviated } \mathrm{KHP}\right)$ with 20.46 $\mathrm{mL}$ of a 0.1000-M NaOH solution. KHP (molar mass 5 204.22 g/ mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

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