Question

Determine the pH of a solution that is 0.15 M NaH2PO4 and 0.10 M Na2HPO4 (the...

Determine the pH of a solution that is 0.15 M NaH2PO4 and 0.10 M Na2HPO4 (the Ka for H2PO4- is 6.2 x10^-8). Include a chemical equation showing the relevant equilibrium.

Please show me how you got the answer, I understand how to do single pH calculations but not entirely sure how to do it with two chemicals. Thanks!

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
Calculate the pH of: 1) .10 M Na2HPO4 2) .10 M NaH2PO4 Teacher's hints: The pH...
Calculate the pH of: 1) .10 M Na2HPO4 2) .10 M NaH2PO4 Teacher's hints: The pH of any intermediate salt of a polyprotic acid is independent of concentration. It will equal the average of the pKa's, according to the formula pH=1/2 (pKa1 + pKa2). I'm not sure what pKas to use.
a) What is the pH of 0.10 M NaH2PO4? Ka2 = 6.2 x 10-8 b) What...
a) What is the pH of 0.10 M NaH2PO4? Ka2 = 6.2 x 10-8 b) What is the pH of 0.10 M Na2​HPO4? Ka3 = 2.2 x 10-13
Set up the equilibrium equation and determine the pH of the 0.15 M solution of potassium...
Set up the equilibrium equation and determine the pH of the 0.15 M solution of potassium nitrate? (Ka value for nitrous acid= 4.0x 10-4).
A 45.0 mL buffer solution is 0.430 M Na2HPO4 (aq) and 0.330 M KH2PO4 (aq). The...
A 45.0 mL buffer solution is 0.430 M Na2HPO4 (aq) and 0.330 M KH2PO4 (aq). The ka for H2PO4- is 6.2*10-8 a. what is the pH of the buffer solution b. what are the pH and the pH change resulting from the addition of 9.0*10-4 mol of NaOH to the buffer solution c. what are the pH and the pH change resulting from the addition of 9.5*10-4 mol of nitric acid to the initial buffer system d. how many mL...
0.10 M Phospate buffer at pH 7.0 total 100.0 ml. 30mL of 0.20M NaH2PO4, 20 mL...
0.10 M Phospate buffer at pH 7.0 total 100.0 ml. 30mL of 0.20M NaH2PO4, 20 mL of 0.20M Na2HPO4 and 50.0 mL of water were used to prepare the buffer. The average pKa is 6.76 Using the average pKa value calculated in 3, calculate the pH of the pH 7.0 buffer solution that is expected after the addition of 1.0 mL of 1.0M HCl.
A) Need to prepare 100 ml of a 0.10 M phosphate buffer with a pH of...
A) Need to prepare 100 ml of a 0.10 M phosphate buffer with a pH of 6.2. Calculate the amounts of 1.0 M NaH2PO4 and 1.0 M K2HPO4 solutions which will give the required pH of 6.2.Use the Henderson-Hasselbalch equation ( pH = pKa + log (base/acid) B) Need to prepare 100 ml of a solution containing 0.025 M NaHCO3 and 0.12 M NaHCO3 and 0.12 M NaCl From stock solutions of 0.05 M NaHCO3 and 0.24 M NaCl from...
What is the pH of a 0.15 M solution of HClO? Ka for HClO = 3.5...
What is the pH of a 0.15 M solution of HClO? Ka for HClO = 3.5 x 10-8   The value of Ka for the weak acid Benzoic acid (C6H6COOH) is 1.5 × 10-5. What are the equilibrium concentrations of all species if 1.50 g of Benzoic acid is dissolved in enough water to make a 250.0 mL solution? What is the pH of the solution? Ammonium ion is the conjugate acid of Ammonia.   What is the pH of a 0.25...
Consider the titration of 25mL of 0.10 M HNO2 with 0.15 M NaOH. The Ka of...
Consider the titration of 25mL of 0.10 M HNO2 with 0.15 M NaOH. The Ka of nitrous acid is 4.0 X 10^-4. a) Write the balanced equation for the neutralization reaction. b) What is the pH of the acid solution before addition of any NaOH? c) How many milliliters of NaOH are required to reach the equivalence point? d) What is the pH at the halfway point of the titration? e) Will the pH at the equivalence be less than...
A buffer solution is prepared from 5.74 g of NH4NO3 and 0.10 L of 0.15-M NH3....
A buffer solution is prepared from 5.74 g of NH4NO3 and 0.10 L of 0.15-M NH3. Calculate the pH of the solution. Ka(ammonium) = 5.6 × 10-10
Consider a buffer solution that contains 0.30 M H3PO4 and 0.10 M NaH2PO4. pKa(H3PO4)=2.16. 1. Calculate...
Consider a buffer solution that contains 0.30 M H3PO4 and 0.10 M NaH2PO4. pKa(H3PO4)=2.16. 1. Calculate its pH 2. Calculate the change in pH if 0.150 g of solid NaOH is added to 200 mL of this solution. 3. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT