Question

A solution of Na2CO3 has a pH of 10. The CO32- ion is the conjugate base...

A solution of Na2CO3 has a pH of 10. The CO32- ion is the conjugate base of the HCO3- ion.

a. Describe these ions using the Bronsted-Lowry definition of an acid and base (use labels AND explain).

b. Write a net ionic equation for the reaction that makes a solution of Na2CO3 basic.

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
Acrylic acid is the conjugate acid of the weak base sodium acrylate, NaC3H3O2. The Ka for...
Acrylic acid is the conjugate acid of the weak base sodium acrylate, NaC3H3O2. The Ka for acrylic acid is 5.5 X 10-5. Using this information, complete the following: (3 points) A.) Write a balanced net ionic equation for the reaction of the acrylate anion with water, which illustrates why this reaction makes the solution basic. B.) Calculate Kb for this reaction C.) Find the pH of a solution prepared by dissolving 1.61 g of sodium acrylate in enough water to...
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...
Design a buffer that has a pH of 3.73 using one of the weak acid/conjugate base...
Design a buffer that has a pH of 3.73 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 × 10-5 4.19 H2PO4- HPO42- 6.2 × 10-8 7.21 HCO3- CO32- 4.8 × 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M...
Design a buffer that has a pH of 6.66 using one of the weak acid/conjugate base...
Design a buffer that has a pH of 6.66 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4×10-5 4.19 H2PO4- HPO42- 6.2×10-8 7.21 HCO3- CO32- 4.8×10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium...
Design a buffer that has a pH of 6.65 using one of the weak acid/conjugate base...
Design a buffer that has a pH of 6.65 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4×10-5 4.19 H2PO4- HPO42- 6.2×10-8 7.21 HCO3- CO32- 4.8×10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams sodium...
A buffer is a mixed solution of a weak acid or base, combined with its conjugate....
A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift...
Question: Consider a .045 M solution of benzoic acid (C6H5CO2H) whose Ka value is 6.5 x...
Question: Consider a .045 M solution of benzoic acid (C6H5CO2H) whose Ka value is 6.5 x 10-5. A). write the acid-base reaction equation for this acid with water: B). write the equilibrium expression (Ka) for this reaction: C). Calculate the concentration of benzoic acid, benzoate ion (the conjugate base), and hydronium ion for this solution. D). Calculate the pH of this solution. E). Calculate the concentration of hydroxide ions in this solution.
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base...
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the addedH+, forming more...
1)Design a buffer that has a pH of 10.12 using one of the weak base/conjugate acid...
1)Design a buffer that has a pH of 10.12 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pKa CH3NH2 4.2×10-4 CH3NH3+ 2.4×10-11 10.62 C6H15O3N 5.9×10-7 C6H15O3NH+ 1.7×10-8 7.77 C5H5N 1.5×10-9 C5H5NH+ 6.7×10-6 5.17 How many grams of the bromide salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams bromide...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT