Question

Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq)...

Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq) + H3O+(aq) In a 0.200 M aqueous solution of HCNO, the concentration of H3O+ is 6.50 x 10-3M. The equilibrium constant (Kc) for this reaction is?

Homework Answers

Answer #1

HCNO(aq) + H2O(l) <---------------------->   CNO-(aq) + H3O+(aq)

0.200                                                    6.50 x 10-3 6.50 x 10-3

[CNO-] = [H3O+]

Kc = [CNO-] [H3O+] / [HCNO]   

Kc = ( 6.50 x 10^-3)^2 / 0.200

Kc = 2.11 x 10^-4

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq)...
Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq) + H3O+(aq) In a 0.200 M aqueous solution of HCNO, the concentration of H3O+ is 6.50 x 10-3M. The equilibrium constant (Kc) for this reaction is
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.260 M HC2H3O2,...
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.260 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25∘C?
For the reaction HF(aq) + H2O (l) <--->    H3O+(aq) + F-(aq)      Kc = 6.8...
For the reaction HF(aq) + H2O (l) <--->    H3O+(aq) + F-(aq)      Kc = 6.8 x 10-4 What is [H3O+] at equilibrium for a 0.0100M solution of HF. ( successive approximation method or quadratic) ( 2 sig figs)
Calculate the pH of a buffer solution prepared by dissolving 0.200 mole of cyanic acid (HCNO)...
Calculate the pH of a buffer solution prepared by dissolving 0.200 mole of cyanic acid (HCNO) and 0.800 mole of sodium cyanate (NaCNO) in enough water to make 1.00 liters of solution. Ka(HCNO) = 2.0 x 10-4 A. 3.70 B. 4.40 C. 3.10 D. 4.30
The equilibrium constant, Ka, for the reaction below is 6.0*10^-3. Fe(H2O)6 ^3+ (aq) + H2O(l) <-->...
The equilibrium constant, Ka, for the reaction below is 6.0*10^-3. Fe(H2O)6 ^3+ (aq) + H2O(l) <--> Fe(H2O)5 (OH)^2+(aq) + H3O^+ (aq) a)Calculate the pH of the 0.10M solution of Fe(H2O)6^3+. b)Will a 1.0 M solution of iron (II) nitrate have a higher or lower pH than a 1.0 M solution of iron (III) nitrate?
IF HA IS A WEAK ACID, WHICK EQUILIBRIUM CORRESPONDS TO THE ACID EQUILIBRIUM CONSTANT Ka for...
IF HA IS A WEAK ACID, WHICK EQUILIBRIUM CORRESPONDS TO THE ACID EQUILIBRIUM CONSTANT Ka for Ha? a. HA (aq) + H2O (l)<--->H2A+ (aq) + OH- (aq) b. A- (aq) + H3O+ (aq)<---> HA (aq) + H2O (l) c. HA (aq) + OH-(aq)<---> H2O (l) + H+ (aq) d. A- (aq) +H2 O (l)<---> HA (aq) + OH- (aq) e. A- (aq) + OH- (aq)<---> HOA2- (aq)
a.) Phosphoric acid is a triprotic acid: H3PO4(aq) +H2O(l) ↔ H3O+(aq) + H2PO4-(aq) Ka1 = 7.5...
a.) Phosphoric acid is a triprotic acid: H3PO4(aq) +H2O(l) ↔ H3O+(aq) + H2PO4-(aq) Ka1 = 7.5 x 10-3 H2PO4-(aq) +H2O(l) ↔ H3O+(aq) + HPO42-(aq) Ka2 = 6.2 x 10-8 HPO42-(aq) +H2O(l) ↔ H3O+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Determine whether sodium monohydrogen phosphate (Na2HPO4) is neutral, basic, or acidic. First, what is its Ka when it acts as an acid? b.) Second, what is its Kb when it acts as a base? c.) Finally, indicate whether the HPO42-...
In-Class Assignment #6 (ch. 18) [10 pts.] CH3COOH (aq)  +  H2O(l)    ⇌   H3O+(aq) + CH3COO−(aq)       ...
In-Class Assignment #6 (ch. 18) [10 pts.] CH3COOH (aq)  +  H2O(l)    ⇌   H3O+(aq) + CH3COO−(aq)        Ka = 1.8 x 10-5 For the reaction of above, write the expression for Ka. Set up an ICE table and find [H3O+] for a 0.10 M solution of CH3COOH. Calculate the pH of the solution at equilibrium
Oxalic acid can donate two protons to water in successive reactions: (1) H2C2O4(aq)+H2O(l)⇌H3O+(aq)+HC2O4-(aq) (2) HC2O4-(aq)+H2O(l)⇌H3O+(aq)+C2O42-(aq) If...
Oxalic acid can donate two protons to water in successive reactions: (1) H2C2O4(aq)+H2O(l)⇌H3O+(aq)+HC2O4-(aq) (2) HC2O4-(aq)+H2O(l)⇌H3O+(aq)+C2O42-(aq) If Kc1 = 5.9 × 10-2 andKc2 = 6.4 × 10-5 at 25°C, what is the value of Kc for reaction (3)? (3) H2C2O4(aq)+2H2O(l)⇌2H3O+(aq)+C2O42-(aq) A) 9.2 × 102 B) 1.1 × 10-3 C) 5.9 × 10-2 D) 3.8 × 10-6 Why is C not the right answer? Does Hess's Law not apply in this problem?
Given the equilibrium reactions: #1) SO2(aq) + H2O(l) = HSO3- (aq) + H+(aq) #2) HSO3- (aq)...
Given the equilibrium reactions: #1) SO2(aq) + H2O(l) = HSO3- (aq) + H+(aq) #2) HSO3- (aq) + H+(aq) = SO32- + 2H+(aq) What is the equilibrium constant for reaction #1 if the concentration of SO2 is 8.50E-20 M, SO32- is 0.619 M, and H+ is 2.00E-07 M? You know that the equilibrium constant (K) for reaction #2 is 130.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT