14th Edition

ISBN: 9780134863016

Author: Brown

Publisher: PEARSON

Concept explainers

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibri…

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Videos

Textbook Question

Chapter 16.6, Problem 16.14.2PE

Practice Exercise 2

Calculate the pH of a 0.020 M solution of oxalic acid (H₂C₂O₄). (See Table 16.3 for K_a₁ and K_a₂.)
Calculate the concentration of oxalate ion, [C₂O₄²^-], in this solution.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 16.6, Problem 16.14.1PE

Chapter 16.7, Problem 16.15.1PE

Students have asked these similar questions

EXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.

Exercise 1 Calculate the pH of each of the following solutions: (a) 0.63 M NaCH3CO2(aq), K, = 5.62 × 10-10, %3D (b) 0.19 M NH4CI(aq), K, = 5.6 × 10-10; %3D (c) 0.65 M KCN(aq), K½ = 2 × 10-5.

Exercise 3. ldentify all the Bronsted acids and bases in the following equations: (a) NH3 + HCI NH,* + CH (b) HSO; + CN- HCN + SO,- (c) H,PO, + CO;- HPO,2- + HCO;

Chapter 16 Solutions

CHEMISTRY THE CENTRAL SCIENCE 14TH EDI

Ch. 16.2 - Practice Exercise 1 Consider the following...Ch. 16.2 - Prob. 16.1.2PE Ch. 16.2 - Prob. 16.2.1PE Ch. 16.2 - Practice Exercise 2 When lithium oxide (Li2O) is...Ch. 16.2 - Based on information in Figure 16.4, place the...Ch. 16.2 - Practice Exercise 2 For each reaction, use Figure...Ch. 16.3 - Practice Exercise 1 In a certain acidic solution...Ch. 16.3 - Practice Exercise 2 Indicate whether solutions...Ch. 16.3 - Prob. 16.5.1PE Ch. 16.3 - Prob. 16.5.2PE

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Practice Exercise 2 Calculate the pH of a 0.020 M solution of oxalic acid (H 2 C 2 O 4 ). (See Table 16.3 for K a 1 and K a 2 .) Calculate the concentration of oxalate ion, [C 2 O 4 2 - ], in this solution.

Concept explainers

Videos

Want to see the full answer?

Chapter 16 Solutions