Question

A mixture formed by adding 49.0 mL of 1.5×10−2 M HCl to 130 mL of 1.5×10−2...

A mixture formed by adding 49.0 mL of 1.5×10−2 M HCl to 130 mL of 1.5×10−2 M HI .

Express the pH of the solution to two decimal places.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Both HCl and HI are strong acids.
Number of moles of hydrogen ion from 49.0 mL of M   HCl =   moles
Number of moles of hydrogen ion from 130 mL of M HI   moles
Total number of moles of hydrogen ions moles
Total volume


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 each of the following strong acid solutions. 1. 20.00 mL of 1.50...
Calculate the pH of each of the following strong acid solutions. 1. 20.00 mL of 1.50 M  HCl diluted to 0.480 L . Express the pH of the solution to three decimal places. 2. A mixture formed by adding 46.0 mL of 2.5×10−2M  HCl to 120 mL of 1.5×10−2M  HI. Express the pH of the solution to two decimal places.
Calculate pH: 5.00 mL of 1.20 M  HCl diluted to 0.440 L & A mixture formed by...
Calculate pH: 5.00 mL of 1.20 M  HCl diluted to 0.440 L & A mixture formed by adding 42.0 mL of 1.5×10−2M  HCl to 160 mL of 1.0×10−2M  HI. The equilibrium constant Kc for C(s)+CO2(g)⇌2CO(g) is 1.9 at 1000 Kand 0.133 at 298 K. How many grams of C are consumed?
Part A 3.41×10−2M  HNO3. Express the pH of the solution to three decimal places. pH = _____...
Part A 3.41×10−2M  HNO3. Express the pH of the solution to three decimal places. pH = _____ Part B 0.260 g of HClO3 in 2.60 L of solution. Express the pH of the solution to three decimal places. pH = _____ Part C 10.00 mL of 1.70 M  HCl diluted to 0.520 L . Express the pH of the solution to three decimal places. pH =_____ Part D A mixture formed by adding 41.0 mL of 2.5×10−2M  HCl to 160 mL of 1.0×10−2M...
Calculate the pH of each of the following strong acid solutions. a. 4.28×10−2 M HNO3. b....
Calculate the pH of each of the following strong acid solutions. a. 4.28×10−2 M HNO3. b. 0.260 g of HClO3 in 2.40 L of solution. c. 20.00 mL of 2.00 M HCl diluted to 0.490 L . d. A mixture formed by adding 57.0 mL of 1.5×10−2 M HCl to 170 mL of 1.0×10−2 M HI.
find pH - answers and work please 2.6×10−2 M HI Express your answer to two decimal...
find pH - answers and work please 2.6×10−2 M HI Express your answer to two decimal places. pH = SubmitMy AnswersGive Up Part B 0.117 M HClO4 Express your answer to three decimal places. pH = SubmitMy AnswersGive Up Part C a solution that is 5.2×10−2 M in HClO4 and 2.8×10−2 M in HCl Express your answer to two decimal places. pH = SubmitMy AnswersGive Up Part D a solution that is 1.90% HCl by mass (Assume a density of...
Problem 16.45 part 2 Part E Calculate [OH−] for 1.60 mL of 0.130 M NaOH diluted...
Problem 16.45 part 2 Part E Calculate [OH−] for 1.60 mL of 0.130 M NaOH diluted to 1.50 L . Express your answer using three significant figures. [OH−] =   M   SubmitMy AnswersGive Up Part F Calculate pH for 1.60 mL of 0.130 M NaOH diluted to 1.50 L . Express your answer using three decimal places. pH = SubmitMy AnswersGive Up Part G Calculate [OH−] for a solution formed by adding 4.70 mL of 0.150 M KOH to 20.0 mL...
Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of 0.100 M...
Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of 0.100 M acetic acid. Acetic acid has a Ka of 1.8 x 10-5. a. Calculate the pH of both solutions before mixing. b. Construct an ICE table representative of this mixture. c. Determine the approximate pH of the solution. d. Determine the percent ionization of the acetic acid in this mixture
Calculate the pH of a solution prepared by adding 20.0 mL of 0.100 M HCl to...
Calculate the pH of a solution prepared by adding 20.0 mL of 0.100 M HCl to 80.0 mL of a buffer that is comprised of 0.25 M CH3NH2 and 0.25 M CH3NH3Cl. Kb of CH3NH2 = 6.8 x 10-5.
Calculate the pH of each of the following strong acid solutions. (a) 0.00458 M HCl pH...
Calculate the pH of each of the following strong acid solutions. (a) 0.00458 M HCl pH = (b) 0.643 g of HClO4 in 37.0 L of solution pH = (c) 60.0 mL of 1.00 M HCl diluted to 4.10 L pH = (d) a mixture formed by adding 69.0 mL of 0.000760 M HCl to 46.0 mL of 0.00882 M HClO4 pH =
A) For 480.0 mL of pure water, calculate the initial pH and the final pH after...
A) For 480.0 mL of pure water, calculate the initial pH and the final pH after adding 0.010 mol of HCl. Express your answers using two decimal places separated by a comma. B) For 480.0 mL of a buffer solution that is 0.150 M in HC2H3O2 and 0.135 M in NaC2H3O2, calculate the initial pH and the final pH after adding 0.010 mol of HCl. Express your answers using two decimal places separated by a comma. C) For 480.0 mL...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT