A containing ammonium chloride was warmed with 150.0 mL of 1.00mol/L sodium hydroxide the ammonia had been driven off, the excess sodium hydroxide required 50.00 mL of 0.150mol/L sulfuric acid for neutralizatior 1. What mass of ammonium chloride did the sample contain?

To determine the mass of ammonium chloride (NH₄Cl) in the sample, we need to follow these steps:1. Calculate the moles of sodium hydroxide (NaOH) used.2. Determine the moles of sulfuric acid (H₂SO₄) used for neutralization.3. Use stoichiometry to find the moles of NH₄Cl.4. Finally, calculate the mass of NH₄Cl.### Step 1: Calculate the moles of NaOHGiven:- Volume of NaOH solution = 150.0 mL = 0.150 L- Concentration of NaOH solution = 1.00 mol/L ### Step 2: Determine the moles of H₂SO₄ used for neutralizationGiven:- Volume of H₂SO₄ solution = 50.00 mL = 0.050 L- Concentration of H₂SO₄ solution = 0.150 mol/L ### Step 3: Use stoichiometry to find the moles of NH₄ClThe balanced chemical equation for the neutralization reaction is: From the equation, 2 moles of NH₄Cl react with 2 moles of NaOH. Therefore, the moles of NH₄Cl are equal to the moles of NaOH used: ### Step 4: Calculate the mass of NH₄ClThe molar mass of NH₄Cl is calculated as follows:- N: 14.01 g/mol- H: 1.01 g/mol (×4 = 4.04 g/mol)- Cl: 35.45 g/mol Now, calculate the mass of NH₄Cl: Therefore, the mass of ammonium chloride in the sample is .