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Chapter 4: Problem 131

A 50.00 -mL sample of aqueous \(\mathrm{Ca}(\mathrm{OH})_{2}\) requires 34.66 \(\mathrm{mL}\) of a 0.944 \(\mathrm{M}\) nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.

Short Answer

Expert verified
The concentration of the original solution of calcium hydroxide is approximately \(0.327 M\).

Step by step solution

01

Write the balanced chemical equation

The balanced chemical equation between calcium hydroxide and nitric acid is: \[Ca(OH)_2 + 2HNO_3 \rightarrow Ca(NO_3)_2 + 2H_2O\]
02

Find the moles of nitric acid used

The volume and concentration of nitric acid used for neutralization are given. We can find the moles of nitric acid using the formula: moles = volume (in L) × concentration (M) volume of nitric acid = 34.66 mL = 0.03466 L concentration of nitric acid = 0.944 M moles of nitric acid = 0.03466 L × 0.944 M = 0.03272104 mol
03

Determine the moles of calcium hydroxide

Now, we'll use the stoichiometry from the balanced chemical equation to find the moles of calcium hydroxide present in the original solution. According to the balanced equation, 1 mole of calcium hydroxide reacts with 2 moles of nitric acid. moles of Ca(OH)_2 = (moles of HNO_3) / 2 moles of Ca(OH)_2 = 0.03272104 mol / 2 = 0.01636052 mol
04

Calculate the concentration of calcium hydroxide

Now that we know the moles of calcium hydroxide and the volume of the original solution (50.00 mL), we can calculate the concentration using the formula: concentration (M) = moles / volume (in L) volume of Ca(OH)_2 = 50.00 mL = 0.0500 L concentration of Ca(OH)_2 = 0.01636052 mol / 0.0500 L = 0.3272104 M The concentration of the original solution of calcium hydroxide is approximately \(0.327 M\).

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Most popular questions from this chapter

Citric acid, which can be obtained from lemon juice, has the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\) . A 0.250 -g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride is mixed with 100.0 mL of a 0.100-M solution of iron(III) sulfate?

Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction is $$\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{MnCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cl}_{2}(g)$$ Balance this equation.

Tris(pentafluorophenyl)borane, commonly known by its acronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?

A stream flows at a rate of \(5.00 \times 10^{4}\) liters per second (L/s) upstream of a manufacturing plant. The plant discharges $3.50 \times 10^{3} \mathrm{L} / \mathrm{s}\( of water that contains 65.0 \)\mathrm{ppm} \mathrm{HCl}$ into the stream. (See Exercise 135 for definitions.) a. Calculate the stream's total flow rate downstream from this plant. b. Calculate the concentration of \(\mathrm{HCl}\) in ppm downstream from this plant. c. Further downstream, another manufacturing plant diverts $1.80 \times 10^{4} \mathrm{L} / \mathrm{s}$ of water from the stream for its own use. This plant must first neutralize the acid and does so by adding lime: $$\mathrm{CaO}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(i) $$ What mass of CaO is consumed in an 8.00-h work day by this plant? d. The original stream water contained 10.2 \(\mathrm{ppm} \mathrm{Ca}^{2+}\) . Although no calcium was in the waste water from the first plant, the waste water of the second plant contains \(\mathrm{Ca}^{2+}\) from the neutralization process. If 90.0% of the water used by the second plant is returned to the stream, calculate the concentration of \(\mathrm{Ca}^{2+}\) in ppm downstream of the second plant.
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