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Chapter 4: Problem 83

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?

Short Answer

Expert verified
The mass of KHP that reacted completely with the sodium hydroxide solution is \(0.418 \: \text{g}\).

Step by step solution

01

Calculate the moles of NaOH

Using the volume and concentration of NaOH solution, we will calculate the moles of sodium hydroxide: moles of NaOH = volume (L) x concentration (mol/L) First, we need to convert the volume from mL to L: Volume (L) = 20.46 mL × (1 L / 1000 mL) = 0.02046 L Now, we plug the values: moles of NaOH = (0.02046 L)(0.1000 mol/L) = 0.002046 mol
02

Calculate the moles of KHP

The balanced chemical equation for the titration reaction between KHP and NaOH is: KHP + NaOH → NaKP + H₂O From this equation, we can see that the reaction is in a 1:1 ratio, meaning 1 mole of KHP reacts with 1 mole of NaOH. Therefore, the moles of KHP that reacted are equal to the moles of NaOH: moles of KHP = moles of NaOH = 0.002046 mol
03

Calculate the mass of KHP that reacted

Now that we have the moles of KHP, we will convert it to mass using the molar mass of KHP (204.22 g/mol): mass of KHP = moles of KHP × molar mass mass of KHP = (0.002046 mol)(204.22 g/mol) = 0.418 g So, the mass of KHP that reacted completely with the sodium hydroxide solution is 0.418 g.

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Most popular questions from this chapter

Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.

What mass of solid AgBr is produced when 100.0 \(\mathrm{mL}\) of 0.150 \(\mathrm{MAgNO}_{3}\) is added to 20.0 \(\mathrm{mL}\) of 1.00 $\mathrm{M} \mathrm{NaBr} ?$

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