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Chapter 4: Problem 103

(a) A strontium hydroxide solution is prepared by dissolving 12.50 g of \(\operatorname{Sr}(\mathrm{OH})_{2}\) in water to make 50.00 \(\mathrm{mL}\) of solution. What is the molarity of this solution? (b) Next the strontium hydroxide solution prepared in part (a) is used to titrate a nitric acid solution of unknown concentration. Write a balanced chemical equation to represent the reaction between strontium hydroxide and nitric acid solutions. (c) If 23.9 mL of the strontium hydroxide solution was needed to neutralize a 37.5 mL aliquot of the nitric acid solution, what is the concentration (molarity) of the acid?

Short Answer

Expert verified
(a) The molarity of the strontium hydroxide solution is 2.054 M. (b) The balanced chemical equation for the reaction between strontium hydroxide and nitric acid solutions is: Sr(OH)\(_2\) + 2HNO\(_3\) → Sr(NO\(_3\))\(_2\) + 2H\(_2\)O. (c) The concentration (molarity) of the nitric acid solution is 2.4856 M.

Step by step solution

01

Calculate the molarity of strontium hydroxide solution

To calculate the molarity of the solution, we first need to determine the moles of the solute (Sr(OH)\(_2\)). Then divide the moles by the volume of the solution. 1. Calculate the moles of Sr(OH)\(_2\): \[Sr(OH)_2 = 1 \times (87.62) + 2 \times (15.999 + 1.008)\] \[Sr(OH)_2 = 87.62 + 2 \times (16.997)\] \[Sr(OH)_2 = 121.62\] moles = grams / molar mass = 12.50 g / 121.62 g/mol = 0.1027 mol 2. Molarity of strontium hydroxide solution: Molarity (M) = moles / volume in L M = 0.1027 mol / 50.00 mL * \(\frac{1L}{1000mL}\) = 2.054 M
02

Write the balanced chemical equation

To write the balanced chemical equation for the reaction between strontium hydroxide (Sr(OH)\(_2\)) and nitric acid (HNO\(_3\)), we must ensure that the number of atoms for each element on the reactants side equals the number of atoms for each element on the products side. Chemical Equation: Sr(OH)\(_2\) + 2HNO\(_3\) → Sr(NO\(_3\))\(_2\) + 2H\(_2\)O
03

Calculate the concentration of nitric acid

We will now use the volume of the strontium hydroxide solution needed to neutralize a 37.5 mL aliquot of the nitric acid solution to determine the concentration (molarity) of the nitric acid. For this, the balanced chemical equation (from Step 2) and the stoichiometry will be used. From the balanced equation, 1 mole of Sr(OH)\(_2\) reacts with 2 moles of HNO\(_3\). 1. Moles of Sr(OH)\(_2\) in the 23.9 mL solution: moles = M * volume in L, moles = 2.054 M * 23.9 mL * \(\frac{1L}{1000mL}\)= 0.0466 mol 2. Calculate moles of HNO\(_3\): 2 moles of HNO\(_3\) react with 1 mole of Sr(OH)\(_2\): moles of HNO\(_3\) = 2 * moles of Sr(OH)\(_2\) moles of HNO\(_3\) = 2 * 0.0466 mol moles of HNO\(_3\) = 0.0932 mol 3. Molarity of nitric acid solution: Molarity (M) = moles / volume in L, M = 0.0932 mol / 37.5 mL * \(\frac{1L}{1000mL}\) = 2.4856 M

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Most popular questions from this chapter

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: $$\begin{array}{c}{\mathrm{Br}_{2}(a q)+2 \mathrm{Nal}(a q) \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q)} \\ {\mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q)}\end{array}$$ (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides? (b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed. (c) Predict whether a reaction will occur when elemental bromine and lithium chloride are mixed.

(a) How many milliliters of 0.120 \(\mathrm{M}\) HCl are needed to completely neutralize 50.0 \(\mathrm{mL}\) of 0.101 \(\mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution? (b) How many milliliters of 0.125 \(\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) are needed to neutralize 0.200 \(\mathrm{g}\) of NaOH? \((\mathrm{c})\) If 55.8 \(\mathrm{mL}\) of a BaCl \(_{2}\) solution is needed to precipitate all the sulfate ion in a 752 -mg sample of \(\mathrm{Na}_{2} \mathrm{SO}_{4},\) what is the molarity of the BaCl\(_{2}\) solution?

(a) What volume of 0.115 \(\mathrm{M} \mathrm{HClO}_{4}\) solution is needed to neutralize 50.00 \(\mathrm{mL}\) of 0.0875 \(\mathrm{M} \mathrm{NaOH} ?(\mathbf{b})\) What volume of 25.8 \(\mathrm{mL}\) of an AgNO \(_{3}\) solution is needed to precipitate all the \(\mathrm{Cl}^{-}\) ions in a 785 -mg sample of \(\mathrm{KCl}\) (forming AgCl), what is the molarity of the AgNO \(_{3}\) solution? (d) If 45.3 \(\mathrm{mL}\) of a 0.108 \(M \mathrm{HCl}\) solution is needed to neutralize a solution of \(\mathrm{KOH}\) , how many grams of \(\mathrm{KOH}\) must be present in the solution?

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile,\(\mathrm{CH}_{3} \mathrm{CN},(\mathbf{c}) \mathrm{NaClO}_{4},(\mathbf{d}) \mathrm{Ba}(\mathrm{OH})_{2} .\)

Separate samples of a solution of an unknown salt are treated with dilute solutions of \(\mathrm{HBr}, \mathrm{H}_{2} \mathrm{SO}_{4},\) and \(\mathrm{NaOH} .\) A precipitate forms in all three cases. Which of the following cations could be present in the unknown salt solution: \(\mathrm{K}^{+}, \mathrm{Pb}^{2+}, \mathrm{Ba}^{2+}.\)
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