What is the pH of a solution of 1.4 M HF in 1.9 M CaF2? (Ka HF = 7.2 x 10-4) %3D IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Include the sign if your answer is negative (not necessary for positive values) • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the significant figures) • Correctly round your answer to the 2nd decimal place (margin of allowed error is only + 0.01, so always use un-rounded numbers in your calculations). If the last digits are zeros they will not display once you click away, but the answer will still be marked correct. Examples: 12.34 or -0.56

What is the pH of a solution of 1.4 M HF in 1.9 M CaF2? (Ka HF = 7.2 x 10-4) %3D IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Include the sign if your answer is negative (not necessary for positive values) • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the significant figures) • Correctly round your answer to the 2nd decimal place (margin of allowed error is only + 0.01, so always use un-rounded numbers in your calculations). If the last digits are zeros they will not display once you click away, but the answer will still be marked correct. Examples: 12.34 or -0.56

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Q20 Given: K₁ of HF 6.8 x 10-4 Ka of NH4 = 6.3 × 10-¹0 Ka of HCN= 4.9 × 10-¹0 According to the given data above, a 0.10 M solution of which of the following would have the highest pH? NaF, NaCN, NH4C1, NH4F, NH4CN =
A student is titrating 150.0 mL of a 0.300 M solution of lactic acid (pKa of lactic acid is 3.85) with a 0.250 M solution of NaOH. What volume of NaOH is needed to reach the equivalence point? Is the solution at the equivalence point acidic, basic, or neutral? L of 0.250 M NaOH Circle one: acidic basic neutral Calculate the pH at the equivalence point. Round your answer to 2 decimal places. pH =
Parts A-C (These are NOT graded, this is prep work to learn do a lab assignment so I can do the actual lab correctly)
What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOOK? Ka of HCOOH is 1.7 x 10-4 (Round-off your final answer in two decimal place)
#3. a. Determine the [OH−] , pH, and pOH of a solution with a [H+] of 9.5×10−13 M at 25 °C. b. Determine the [H+] , pH, and pOH of a solution with an [OH−] of 9.4×10−8 M at 25 °C. c. Determine the [H+] , [OH−] , and pOH of a solution with a pH of 13.38 at 25 °C. d. Determine the [H+] , [OH−] , and pH of a solution with a pOH of 10.89 at 25 °C.
Answer all parts
Which acid ionization constant would indicate the weakest acid? Group of answer choices 3.5 x 10–4 1.8 x 10–5 4.6 x 10–4 1.5 x 10–2
plese don't handwritten solution..
9:07 AM Wed Mar 1 Question 15 of 26 What volume (in mL) of 9.2 M HCIO4 would be required to make 500.0 mL of a solution with a pH of 3.20? Tap here or pull up for additional resources
0 A certain weak base has a K₁ of 7.40 × 10-7. What concentration of this base will produce a pH of 10.15? concentration: 11.35 Incorrect M
Write the pH value for solutions with the following H30+ concentrations (provide an answer for all three). a) 6 x 10-11 M b) 2 x 10-8 M c) 5 x 10-5 M U S X2 В I
15