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Chapter 4: Problem 37

What mass of NaOH is contained in 250.0 mL of a 0.400 M sodium hydroxide solution?

Short Answer

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

Step by step solution

01

Find the number of moles of NaOH contained in the solution

To calculate the number of moles of NaOH in the solution, we can use the formula: number of moles = molarity × volume Since we know the molarity (0.400 M) and volume (250.0 mL), we can plug these values into the formula: number of moles = 0.400 mol/L × 0.250 L Note that we need to convert the volume from milliliters to liters by dividing by 1000 (1 L = 1000 mL).
02

Calculate the number of moles of NaOH

Now we can multiply the molarity and volume to find the number of moles of NaOH: number of moles = 0.400 mol/L × 0.250 L = 0.100 mol
03

Calculate the molar mass of NaOH

To convert the number of moles of NaOH to mass, we need to know the molar mass of NaOH. The molar mass can be found by adding the molar masses of each element in the compound: Molar mass of NaOH = molar mass of Na + molar mass of O + molar mass of H Using the periodic table, we can find the molar masses of each element: - Molar mass of Na = 22.99 g/mol - Molar mass of O = 16.00 g/mol - Molar mass of H = 1.01 g/mol So, the molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol
04

Calculate the mass of NaOH in the solution

Now that we have the molar mass of NaOH and the number of moles present in the solution, we can calculate the mass of NaOH using the formula: mass = number of moles × molar mass mass of NaOH = 0.100 mol × 40.00 g/mol = 4.00 g So, there are 4.00 grams of NaOH contained in 250.0 mL of a 0.400 M sodium hydroxide solution.

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Most popular questions from this chapter

What volume of 0.100\(M \mathrm{NaOH}\) is required to precipitate all of the nickel(Il) ions from 150.0 \(\mathrm{mL}\) of a \(0.249-M\) solution of \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2} ?\)

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?

When organic compounds containing sulfur are bumed, sulfur dioxide is produced. The amount of \(\mathrm{SO}_{2}\) formed can be determined by the reaction with hydrogen peroxide: $$\mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{SO}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)$$ The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.302 -g sample of coal is burned and the \(\mathrm{SO}_{2}\) is collected in a solution of hydrogen peroxide. It took 28.44 \(\mathrm{mL}\) of a $0.1000-M \mathrm{NaOH}$ solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.

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.

Three students were asked to find the identity of the metal in a particular sulfate salt. They dissolved a 0.1472-g sample of the salt in water and treated it with excess barium chloride, resulting in the precipitation of barium sulfate. After the precipitate had been filtered and dried, it weighed 0.2327 g. Each student analyzed the data independently and came to different conclusions. Pat decided that the metal was titanium. Chris thought it was sodium. Randy reported that it was gallium. What formula did each student assign to the sulfate salt? Look for information on the sulfates of gallium, sodium, and titanium in this text and reference books such as the CRC Handbook of Chemistry and Physics. What further tests would you suggest to determine which student is most likely correct?
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