Question

Part A The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq) Which...

Part A The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq) Which of the following represents a conjugate acid-base pair? The following equation shows the equilibrium in an aqueous solution of ammonia: Which of the following represents a conjugate acid-base pair? NH3 and H2O NH4+ and OH− H2O and OH− NH3 and OH−

Part Part B What is the conjugate base of HCO3−? Express your answer as a chemical formula.

Part Part C What is the conjugate acid of HPO22− ? Express your answer as a chemical formula.

Part Part D Among three bases, X−, Y−, and Z−, the strongest one is Y−, and the weakest one is Z−. Rank their conjugate acids, HX, HY, and HZ, in order of decreasing strength. Rank the acids from strongest to weakest. To rank items as equivalent, overlap them. HelpReset HZHYHX Weakest acidStrongest acid The correct ranking cannot be determined.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Ammonia is a weak base that reacts with water according to this equation: NH3(aq)+H2O(l)<-->NH4+ + OH-(aq)....
Ammonia is a weak base that reacts with water according to this equation: NH3(aq)+H2O(l)<-->NH4+ + OH-(aq). Will any of of the following incrase the percentage of ammonia that is converted to the ammonium ion in water. a) Addition of NaOH b) Addition of HCl c) Addition of NH4Cl
You have found the following: NH3(aq) + H2O(l) <=> OH-(aq) + NH4+(aq) K = (1.8991x10^-5) OH-(aq)...
You have found the following: NH3(aq) + H2O(l) <=> OH-(aq) + NH4+(aq) K = (1.8991x10^-5) OH-(aq) + H+(aq) <=> H2O(l) K = (1.067x10^14) What is the value of K for the following reaction? NH3(aq) + H+(aq) <=> NH4+(aq)
For the following equation label the conjugate acid-base pairs. HC2H3O2 + NH3 <===> NH4+ + C2H3O2-...
For the following equation label the conjugate acid-base pairs. HC2H3O2 + NH3 <===> NH4+ + C2H3O2- 2. The formation of products is strongly favored in this acid-base system: HX + B- <===> HB + X- a) Identify the bases competing for protons. b) Which is the weaker acid in the above equation? Explain. c) Which base is the stronger? Explain. d) How would the equilibrium be affected by the addition of the soluble salt, NaB? e) Would the Keq for...
The salt ammonium nitrate, NH4NO3(s), completely dissociates into NH4+(aq) and NO3−(aq) in an aqueous environment. The...
The salt ammonium nitrate, NH4NO3(s), completely dissociates into NH4+(aq) and NO3−(aq) in an aqueous environment. The NO3−ion has no acid or base properties, but the ammonium ion is the conjugate acid of the weak base, ammonia. Part a. Write a balanced chemical equation showing how the ammonium ion reacts with water to affect the pH of the resulting solution (you can ignore the nitrate ion in your balanced equation). Part b. Find the pH of a 0.100 M solution of...
Which of the following statements involving ammonia is false ? at the equivalence point of a...
Which of the following statements involving ammonia is false ? at the equivalence point of a titration of aqueous NH3 with aqueous HCl, the pH should be > 7 ammonia can act as a Brønsted-Lowry base or a Lewis base ammonia is a stronger base than H2O, but ammonia is a weaker base than OH− store-bought aqueous NH3 has a pungent smell because NH3 does not completely hydrolyze water the following reaction is a Lewis acid-base reaction : Ag+(aq) +...
PART A Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5 and a...
PART A Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5 and a pH of 11.27. What is the percent ionization of ammonia at this concentration? PART B Write a chemical equation for Sr(OH)2(aq) showing how it is an acid or a base according to the Arrhenius definition. PART C Find the pH of the following solutions of mixtures of acid: 0.155 M in HNO2 and 8.5×10−2 M in HNO3
Determine the equilibrium constant for the following solutions: a) H+(aq) + OH-(aq) H2O(l) b) HCl(aq) +...
Determine the equilibrium constant for the following solutions: a) H+(aq) + OH-(aq) H2O(l) b) HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) c) HCN(aq) + KOH(aq) KCN(aq) + H2O(l) d) NH3(aq) + HNO3(aq) NH4NO3(aq)
Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms...
Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized as NX3(aq)+H2O(l)⇌HNX3+(aq)+OH−(aq) where NX3 is the base and HNX3+ is the conjugate acid. The equilibrium-constant expression for this reaction is Kb=[HNX3+][OH−]/[NX3] where Kb is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of Kb increases. Ka and Kb are related through...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
1. Which equilibrium is most important in determining the pH of a solution of sodium phosphate?...
1. Which equilibrium is most important in determining the pH of a solution of sodium phosphate? a. HPO42- + H2O = PO43- + H3O+ b. H2PO42- + H2O = H3PO4 + OH- c. H3PO4 + H2O = H2PO4- + H3O+ d. PO43- + H2O = HPO42- + OH- 2. Tina has two aqueous solutions: 1.2 x 10-2 M NaOH and 1.2 x 10-2 M NH3 (KB=1.8x10-5). Which solution has the higher pH? a. the NaOH solution b. the ammonia solution...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT