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Chapter 4: Problem 1

Household ammonia used for cleaning contains about \(10 \mathrm{~g}\) (two significant figures) of \(\mathrm{NH}_{3}\) in \(100 \mathrm{~mL}\) (two significant figures) of solution. What is the molarity of the \(\mathrm{NH}_{3}\) in solution?

Short Answer

Expert verified
Answer: The molarity of NH3 in the solution is approximately 5.87 M.

Step by step solution

01

Find moles of NH3

First, find the moles of NH3 using the mass and molar mass: Moles of NH3 = mass of NH3 / molar mass of NH3 The mass of NH3 is given as 10 g, and the molar mass of NH3 is 14.01 g/mol for nitrogen and 3 * 1.01 g/mol for three hydrogen atoms, which adds up to 17.03 g/mol. Moles of NH3 = (10 g) / (17.03 g/mol)
02

Calculate the volume of the solution in Liters

We are given that the volume of the solution is 100 mL. To convert this to Liters, we use the conversion factor: 1 L = 1000 mL. Volume in Liters = (100 mL) / (1000 mL/L) = 0.1 L
03

Calculate the molarity of NH3

Now that we have the moles of NH3 and the volume of the solution in Liters, we can find the molarity by dividing the moles by the volume. Molarity of NH3 = moles of NH3 / volume in Liters Molarity of NH3 = (10 g) / [(17.03 g/mol) * (0.1 L)]
04

Solve and report the molarity to the appropriate number of significant figures

When solving the equation above, make sure to consider significant figures. Since both the mass and the volume of the solution are given to two significant figures, the molarity of NH3 should also be reported to two significant figures. Molarity of NH3 ≈ 5.87 M (rounded to two significant figures)

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Most popular questions from this chapter

A capsule of vitamin \(\mathrm{C}\), a weak acid, is analyzed by titrating it with \(0.425 M\) sodium hydroxide. It is found that \(6.20 \mathrm{~mL}\) of base is required to react with a capsule weighing \(0.628 \mathrm{~g}\). What is the percentage of vitamin \(\mathrm{C}\) \(\left(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\right)\) in the capsule? (One mole of vitamin \(\mathrm{C}\) reacts with one mole of hydroxide ion.)

Decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction. (a) potassium nitrate and magnesium sulfate (b) silver nitrate and potassium carbonate (c) ammonium carbonate and cobalt(III) chloride (d) sodium phosphate and barium hydroxide (e) barium nitrate and potassium hydroxide

What is the molarity of each ion present in aqueous solutions prepared by dissolving \(20.00 \mathrm{~g}\) of the following compounds in water to make 4.50 L of solution? (a) cobalt(III) chloride (b) nickel(III) sulfate (c) sodium permanganate (d) iron(II) bromide

Limonite, an ore of iron, is brought into solution in acidic medium and titrated with \(\mathrm{KMnO}_{4}\). The unbalanced equation for the reaction is $$ \mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Fe}^{3+}(a q)+\mathrm{Mn}^{2+}(a q) $$ It is found that a \(1.000-\mathrm{g}\) sample of the ore requires \(75.52 \mathrm{~mL}\) of \(0.0205 \mathrm{M}\) \(\mathrm{KMnO}_{4}\). What is the percent of Fe in the sample?

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