aPure water is a neutral solution and so it always has a pH of 7.b.At 25 °C the pH of pure water is 7Because pure water is neutral the (H3O+]is always equal to the [OH ].Kw = 1.0x10-14 at 25 °CepH = pOH = 7 is only true at 25 °CfAt temperatures above at 25 °C Ky < 1.0×10-14At temperatures above at 25 °C Kw > 1.0x10--14g[3 Fullscreen U16V3 Question 3Homework • UnansweredWhich of the following statements about about water are correct?

a Pure water is a neutral solution and so it always has a pH of 7. b At 25 °C the pH of pure water is 7 Because pure water is neutral the (H30+]is always equal to the [OH¯]. d. Kw 1.0×10-14 at 25 °C %3D pH = pOH = 7 is only true at 25 °C e f At temperatures above at 25 °C Kw < 1.0×10-14 At temperatures above at 25 °C Kw > 1.0×10¬14

a Pure water is a neutral solution and so it always has a pH of 7. b At 25 °C the pH of pure water is 7 Because pure water is neutral the (H30+]is always equal to the [OH¯]. d. Kw 1.0×10-14 at 25 °C %3D pH = pOH = 7 is only true at 25 °C e f At temperatures above at 25 °C Kw < 1.0×10-14 At temperatures above at 25 °C Kw > 1.0×10¬14

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

Calculate the pH for the following concentration: [H,0*] = 2.19 x 10-5 M A. pH=4.7 B. PH=4.9 C. PH= 5.0 D. PH=4.0 Calculate the concentration for the following pH: pH = 13.8 A)[Hg0*] = 1.0 x 10-14 M (B) (H30*] = 1.0 x 104 M (C) (30*] = 1.6 x 1014 M (D) [H30*] = 1.6 x 10-4 M
< Which of the following solutions would be expected to have a pH of 7.00? Weak Acid HCN HNO₂ HIO HBrO C6H5COOH Ka 4.9 x 10-1⁰ 4.5 x 10-4 2.3 x 10-¹1 2.5 x 10-⁹ 6.3 x 10-5 Question 4 of 11 Tap here or pull up for additional resources Weak Base HONH, NH3 CoHsNH, H₂NNH₂ C5H5N A) CSIO B) NaF C) LICIO3 D) KNO₂ Submit
5. When [H+] = 1.0 x 10^-7 M in water at 25°C, then O A. pH = 1 O B. pH = 10^–7. %3D O C. [OH-] = 1.0 × 10^–7 M O D. [OH-] = 1.0 × 10^7 M E. [OH-] = 0 M
Calculate pH when given the following - [OH-]= 3.81 x 10-9M A. pH= 0.000000381 В. рH- 9.22 C. pH= 1.75 D. pH= 7.93 О Е. рH- 5.58
Please don't give handwritten answers
What is the pH of a 0.0235 M H* solution? Formulas [H*] = 10-PH [OH-] = 10-POH H* OH [H]-1x 104 TOH] pH = - log,o[H*] pOH = - log.,[OH-] OH - 14- pH pH + pОН %3D 14 pH РОН pH-14 pOlH -1.63 O 1.63 O 42.66 O 12.37 01-110
Indicate whether solutions with each of the following ion concentrations are neutral, acidic or basic at 25°C (for best practice, try to judge without doing any calculations). - v [OH"] = 7 x 10-13 M A, acidic - [H*] = 4 x 10-9 M B. basic [OH"] = 1 x 10-7 m C. neutral [H*] = 3 x 10-3 M V [OH] = 2 x 10-6 M
1. Arrange the following solution from lowest pH to highest pH: 0.20 М СH,Cоон (Ка - 1.8 х 10-5), 0.06 М СH,соон (Ка - 1.8 х 10-5), 0.75 М сH,COОН (Ка - 1.8х 10-5) %3D 2. Arrange the following solution from lowest pH to highest pH: 0.20 М СН,СОн (Ка 3 1.8 х 10-5), 0.05 M NH, (Kb %3D 1.8 х 10-5), 0.01 М СНООН (Ка 3 1.8 х 10-4) 3. Arrange the following solution from lowest pH to highest pH: 0.20 М СH,СООН (Ка %3D 1.8 х 10-5), 0.20 М НNO, (Ка %3D 4.6 х 10-4), 0.20 М СнОон (Ка 3D 1.8х 10-4) 4. Arrange the following solution from lowest pH to highest pH: 0.75 М СН,СООН (Ка %3D 1.8 х 10-5), 0.01 М HNO, (Ка 3D 4.6 х 10-4), 0.05 М СНООН (Ка 3D 1.8 х 10-4)
Part B Calculate the pH of a mixture containing 3.5x10-2 mol. L-1 HNO3 and 5.1x10-2 mol - L' HCIO. Express your answer to two decimal places. pH = %3D
Trimethylamine, (CH3)3 N, is produced when plants and animals decompose and has a very unpleasant odor. Calculate the [OH ], H*], and pH of a 0.50-M solution of (CH3)3N (K, = 7.4 x 10-5). [OH ] = M [H*] = M pH = %3D