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Chapter 4: Problem 33

What mass of \(\mathrm{NaOH}\) is contained in \(250.0 \mathrm{~mL}\) of a \(0.400 \mathrm{M}\) sodium hydroxide solution?

Short Answer

Expert verified
The mass of NaOH in the 250.0 mL of 0.400 M sodium hydroxide solution is 4.00 grams.

Step by step solution

01

Extract the given values from the problem

We have the following information: Molarity (M) = 0.400 M Volume of the solution (V) = 250.0 mL
02

Convert volume to liters

The volume of the solution should be in liters to use the molarity formula. We can convert the given volume from mL to L by dividing by 1000: \(V = \frac{250.0 \mathrm{~mL}}{1000\mathrm{~mL}} = 0.250 \mathrm{~L}\)
03

Find the moles of NaOH

We can use the molarity formula to find the moles of NaOH, rearranging the formula to solve for moles of solute: moles of solute = Molarity × Volume moles of NaOH = 0.400 M × 0.250 L = 0.100 moles
04

Calculate the molar mass of NaOH

To find the mass of NaOH, we need its molar mass. The molar mass of NaOH can be calculated by adding the molar masses of each of its elements: Molar mass of NaOH = (Molar mass of Na) + (Molar mass of O) + (Molar mass of H) From the periodic table: Molar mass of Na = 22.99 g/mol Molar mass of O = 16.00 g/mol Molar mass of H = 1.01 g/mol Molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol
05

Calculate the mass of NaOH using moles and molar mass

Now, we can find the mass of NaOH in the given solution using the moles of NaOH and the molar mass of NaOH: mass of NaOH = (moles of NaOH) × (molar mass of NaOH) mass of NaOH = 0.100 moles × 40.00 g/mol = 4.00 g The mass of NaOH in the 250.0 mL of 0.400 M sodium hydroxide solution is 4.00 grams.

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Most popular questions from this chapter

Consider the reaction of \(19.0 \mathrm{~g}\) of zinc with excess silver nitrite to produce silver metal and zinc nitrite. The reaction is stopped before all the zinc metal has reacted and \(29.0 \mathrm{~g}\) of solid metal is present. Calculate the mass of each metal in the 29.0-g mixture.

The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every \(10^{6}\) parts of solution. Mathematically, by mass: $$ \mathrm{ppm}=\frac{\mu \mathrm{g} \text { solute }}{\mathrm{g} \text { solution }}=\frac{\mathrm{mg} \text { solute }}{\mathrm{kg} \text { solution }} $$ In the case of very dilute aqueous solutions, a concentration of \(1.0\) ppm is equal to \(1.0 \mu \mathrm{g}\) of solute per \(1.0 \mathrm{~mL}\), which equals \(1.0 \mathrm{~g}\) solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. \(5.0 \mathrm{ppb} \mathrm{Hg}\) in \(\mathrm{H}_{2} \mathrm{O}\) b. \(1.0 \mathrm{ppb} \mathrm{CHCl}_{3}\) in \(\mathrm{H}_{2} \mathrm{O}\) c. \(10.0 \mathrm{ppm}\) As in \(\mathrm{H}_{2} \mathrm{O}\) d. \(0.10 \mathrm{ppm} \mathrm{DDT}\left(\mathrm{C}_{14} \mathrm{H}_{9} \mathrm{Cl}_{5}\right)\) in \(\mathrm{H}_{2} \mathrm{O}\)

Acetylsalicylic acid is the active ingredient in aspirin. It took \(35.17 \mathrm{~mL}\) of \(0.5065 M\) sodium hydroxide to react completely with \(3.210 \mathrm{~g}\) of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

A \(6.50-\mathrm{g}\) sample of a diprotic acid requires \(137.5 \mathrm{~mL}\) of a \(0.750 \mathrm{M} \mathrm{NaOH}\) solution for complete neutralization. Determine the molar mass of the acid.

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\operatorname{CuSO}_{4}(a q)\) b. \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CaCl}_{2}(a q)\) c. \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{Mg} \mathrm{I}_{2}(a q)\) d. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q)+\operatorname{AlBr}_{3}(a q)\)
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