Textbook Question
(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution?
981
views
Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 83
Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resulting solution. The sodium bicarbonate reacts with sulfuric acid according to: 2 NaHCO3(s) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g). Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?
Verified step by step guidance1
Calculate the moles of H2SO4 spilled using the formula: moles = molarity × volume. Convert the volume from mL to L before using it in the calculation.
Use the balanced chemical equation to determine the stoichiometric ratio between H2SO4 and NaHCO3. According to the equation, 1 mole of H2SO4 reacts with 2 moles of NaHCO3.
Calculate the moles of NaHCO3 required by multiplying the moles of H2SO4 by the stoichiometric ratio (2 moles of NaHCO3 per mole of H2SO4).
Determine the mass of NaHCO3 needed using the formula: mass = moles × molar mass. Look up the molar mass of NaHCO3 (sodium bicarbonate) from the periodic table.
Ensure all units are consistent and check calculations for accuracy. The result will give you the minimum mass of NaHCO3 required to neutralize the spilled H2SO4.
Related Practice
Textbook Question
(b) How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.200 g of NaOH?
805
views
Textbook Question
(c) If 55.8 mL of a BaCl2 solution is needed to precipitate all the sulfate ion in a 752-mg sample of Na2SO4, what is the molarity of the BaCl2 solution?
758
views
Textbook Question
The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?
1270
views
Textbook Question
A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide?
1602
views
Textbook Question
A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (b) What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+?
455
views