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Chapter 4: Problem 84

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/ mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.

Short Answer

Expert verified
The molarity of the sodium hydroxide solution is 0.0153 M.

Step by step solution

01

Determine the moles of KHP

To determine the moles of KHP in the sample, we can use the following formula: moles of KHP = mass of KHP / molar mass of KHP We are given the mass of KHP (0.1082 g) and the molar mass of KHP (204.22 g/mol). moles of KHP = 0.1082 g / 204.22 g/mol Calculate the moles of KHP: moles of KHP = \( \frac{0.1082}{204.22} \) = 5.30 x 10^(-4) mol
02

Use stoichiometry to determine the moles of NaOH

From the balanced equation of the reaction between KHP and NaOH, we know that there's a 1:1 ratio of KHP to NaOH: KHP + NaOH → NaKP + H2O So, moles of NaOH = moles of KHP moles of NaOH = 5.30 x 10^(-4) mol
03

Calculate the molarity of the NaOH solution

Now, we will calculate the molarity of the NaOH solution using the moles of NaOH and the given volume of the solution that reacted with the KHP sample (34.67 mL). Remember, molarity (M) is calculated as: Molarity (M) = moles of solute / volume of solution (in liters) We need to convert the volume of NaOH in milliliters to liters before calculating the molarity: volume of NaOH (in L) = 34.67 mL / 1000 = 0.03467 L Now, we can calculate the molarity using the moles of NaOH and volume in liters: Molarity of NaOH = \( \frac{5.30 \times 10^{-4}\,\text{mol}}{0.03467\,\text{L}} \) = 0.0153 M The molarity of the sodium hydroxide solution is 0.0153 M.

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Most popular questions from this chapter

A 30.0 -mL sample of an unknown strong base is neutralized after the addition of 12.0 \(\mathrm{mL}\) of a 0.150 \(\mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.

An average human being has about 5.0 \(\mathrm{L}\) of blood in his or her body. If an average person were to eat 32.0 \(\mathrm{g}\) of sugar (sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}, 342.30 \mathrm{g} / \mathrm{mol}$ ), and all that sugar were dissolved into the bloodstream, how would the molarity of the blood sugar change?

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.

In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution? Assume each solution has a final volume of 100.0 mL. (See Exercise 135 for definitions.)

A solution of permanganate is standardized by titration with oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right) .\) It required 28.97 \(\mathrm{mL}\) of the permanganate solution to react completely with 0.1058 g of oxalic acid. The unbalanced equation for the reaction is $$\mathrm{MnO}_{4}^{-}(a q)+\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q) \stackrel{\mathrm{Acidic}}{\longrightarrow} \mathrm{Mn}^{2+}(a q)+\mathrm{CO}_{2}(g)$$ What is the molarity of the permanganate solution?
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