CHEM 1202 Chapter : Chapter 16 Quiz 3

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azuremammoth471

15 Mar 2019

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Use the chemical structure to determine which of these choices is the strongest base: f, i, no3, hso4, cl- Nh3 is a weak base with the equilibrium constant kb. Hno2 is a weak base with the equilibrium constant ka. Which of the following salt solutions will be the most basic: kbr, nano3, nh4cl, na2co3, nacl. Which of the following salt solutions will be the most acidic: nh4cl, kno3, naf, nacl, kbr. Which of the following salt solutions will be the most basic: nh4cl, kbr, kno3, kcn, nacl. Hclo is a weak acid with the equilibrium constant ka. Which of the salt solutions will be the most basic when equal concentrations of these salt solutions are prepared: nabr, kobr, kbr, kof, nh4cl. Which of the following salt solutions will be the most basic: kno3, naf, nacl, nh4cl, kbr. Hcn is a weak acid with the equilibrium constant ka. Ethlyene amine is a weak base with pkb=5. 99 and the chemical formula c2h5n.

Related Questions

For conjugate acid-base pairs, how are K_a and K_b related?

Consider the reaction of acetic acid in water.

where

a. Which two bases are competing for the proton?

b. Which is the stronger base?

c. In light of your answer to part b, why do we classify the acetate ion (CH₃CO₂^-) as a weak base? Use an appropriate reaction to justify your answer.

In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH₃ is a weak acid.

To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming K_a for a monoprotic strong acid is 1x10⁶, calculate K_b for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li⁺, K⁺, Rb⁺, Cs⁺, Ca²⁺, Sr²⁺, and Ba²⁺ as the conjugate acids of the strong bases LiOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, and Ba(OH)₂. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acid properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a ______ base. The conjugate acid of a weak base is a ______ acid. The conjugate base of a strong acid is a ______ base. The conjugate acid of a strong base is a ______ acid. (Hint: Weak gives you weak and strong gives you worthless.)

limeswan13

Help with Acid/Base equilibrium constant in water!! Withexplanations on how/why!

Need help with Acid/Base water equilibrium reaction withexplanations!!

Please give me explanations on why and how!

1. A solution of 0.05 M of HOClO3 in water has a pH = 1.3 atroom temperature.

a. Write the chemical equation for the acid-base reaction thatoccurs in this solution. What are the conjugate acid and basepairs?

b. Calculate the equilibrium Constant of hydronium/

c. What percent of the acid reacted in solution? Is this astrong or weak acid?

d. Based on the information given, will you expect theequilibrium constant to be greater or less than 1? Why?

2. A solution of 0.1 M of HCN in water has a pH = 3.0 at roomtemperature.

a. Write the chemical equation for the acid-base reaction thatoccurs in this solution. What are the conjugate acid and basepairs?

b. Calculate the equilibrium Constant of hydronium/

c. What percent of the acid reacted in solution? Is this astrong or weak acid?

d. Based on the information given, will you expect theequilibrium constant to be greater or less than 1? Why?

3. 250 mL of an 0.8 M solution of NaD (salt of the weak acid HDwith the Ka of 2.5 * 10^-10) is added to 250 mL of water.

a. What is the chemical reaction?

b. What will be the concentration of D- after dilution?

c. What are the equilibrium expression of Kb for the reaction ofNaD and water?

d. Find the value of the Kb.

Thanks a lot in advance, I'll be sure to rate!

For conjugate acid-base pairs, how are Ka and Kb related?

Consider the reaction of acetic acid in water:

CH₃CO₂H (aq) + H₂O (l) ⇌ CH₃CO₂⁻ (aq) + H₃O⁺ (aq) where Ka = 1.8 × 10⁻⁵

Which two bases are competing for the proton?
Which is the stronger base?
In light of your answer to part b. why do we classify the acetate ion (CH₃CO₂⁻) as a weak base? Use an appropriate reaction to justify your answer.
In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH₃ is a weak acid.

To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1× 10⁶, calculate Kb for the conjugate base of this strong acid.

Why do conjugate bases of strong acids have no basic properties in the water?

List the conjugate bases of the six common strong acids.

To tie it all together, some instructors have students think of Li⁺, K⁺, Rb⁺, Cs⁺, Ca²⁺, Sr²⁺, and Ba²⁺ as the conjugate acids of the strong bases LiOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, and Ba(OH)₂. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. ( Hint: Weak gives you weak and strong gives you worthless.)

periwinklegoat463

CHEM 1202 Chapter : Chapter 16 Quiz 3

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