Skip to main content
Pearson+ LogoPearson+ Logo
Ch.17 - Additional Aspects of Aqueous Equilibria
All textbooksBrown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblem 119b
Chapter 17, Problem 119b

Baking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid (H2CO3), which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO2(g) forms bubbles and causes the cake to rise. (b) The density of baking soda is 2.16 g/cm3. Calculate the concentration of lactic acid in one cup of sour milk (assuming the rule of thumb applies), in units of mol/L. (One cup = 236.6 mL = 48 teaspoons).

Verified step by step guidance
1
Identify the chemical reaction: Sodium bicarbonate (NaHCO3) reacts with lactic acid (C3H6O3) to produce carbonic acid (H2CO3), which decomposes into water (H2O) and carbon dioxide (CO2). The balanced chemical equation is: NaHCO3 + C3H6O3 → NaC3H5O3 + H2CO3.
Determine the molar mass of sodium bicarbonate (NaHCO3) using the periodic table: Na (22.99 g/mol) + H (1.01 g/mol) + C (12.01 g/mol) + 3*O (3*16.00 g/mol) = 84.01 g/mol.
Calculate the mass of baking soda in one teaspoon using its density: Given the density of baking soda is 2.16 g/cm³, and assuming a teaspoon is approximately 5 mL, the mass of baking soda in one teaspoon is 2.16 g/cm³ * 5 cm³ = 10.8 g.
Convert the mass of baking soda to moles: Use the molar mass of NaHCO3 to convert the mass to moles. For example, if you have 10.8 g of NaHCO3, the moles of NaHCO3 = 10.8 g / 84.01 g/mol.
Calculate the concentration of lactic acid in sour milk: Assuming a 1:1 molar ratio between NaHCO3 and lactic acid, the moles of lactic acid will be equal to the moles of NaHCO3. Convert this to molarity by dividing the moles of lactic acid by the volume of sour milk in liters (236.6 mL = 0.2366 L).

Verified Solution

Video duration:
2m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Related Practice
Textbook Question

A concentration of 10–100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Using Ksp values from Appendix D, calculate the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium with (b) AgBr (c) AgI.

986
views
Textbook Question

Fluoridation of drinking water is employed in many places to aid in the prevention of tooth decay. Typically. the Fion concentration is adjusted to about 1 ppm. Some water supplies are also 'hard'; that is, they contain certain cations such as Ca2 + that interfere with the action of soap. Consider a case where the concentration of Ca2 + is 8 ppm. Could a precipitate of CaF2 form under these conditions? (Make any necessary approximations.)

372
views
Textbook Question

Baking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid (H2CO3), which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO2(g) forms bubbles and causes the cake to rise. (a) A rule of thumb in baking is that 1/2 teaspoon of baking soda is neutralized by one cup of sour milk. The acid component in sour milk is lactic acid, CH3CH(OH)COOH. Write the chemical equation for this neutralization reaction.

1562
views
Textbook Question

Baking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid (H2CO3), which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO2(g) forms bubbles and causes the cake to rise.  (c) If 1/2 teaspoon of baking soda is indeed completely neutralized by the lactic acid in sour milk, calculate the volume of carbon dioxide gas that would be produced at 1 atm pressure, in an oven set to 350 F.

9201
views
Textbook Question

In nonaqueous solvents, it is possible to react HF to create H2F+. Which of these statements follows from this observation? (a) HF can act like a strong acid in nonaqueous solvents, (b) HF can act like a base in nonaqueous solvents, (c) HF is thermodynamically unstable, (d) There is an acid in the nonaqueous medium that is a stronger acid than HF.

597
views