4) Which of the following pH values indicate a neutral solution?
(a) pH=2 (b) pH=5 (c) pH=7 (d) pH=9
5) Which of the following forms a solution with a pH of 13.7?
(a)0.02M solution of NaOH (b) 0.04M solution of Mg(OH)2 (c) 0.2M solution of HCl (d) 0.5M solution of NaOH
6) Which of the following forms a solution with a pH of 13?
(a) 0.01M solution of NaOH (b) 0.03M solution of HCl (c) 0.05M solution of Ba(OH)2 (d) 0.05M solution of NaOH
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4) Which of the following pH values indicate a neutral solution? (a) pH=2 (b) pH=5 (c)...
Question 18 Which of the following forms a solution with a pH of 13.7? (1 point) 0.02M solution of NaOH 0.04M solution of Mg(OH)2 O 0.2M solution of HCI O 0.5M solution of NaOH Question 19 Which of the following forms a solution with a pH of 13? (1 point) O 0.01M solution of NaOH 0.03M solution of HCI 0.05M solution of Ba(OH)2 0.05M solution of NaOH
Question 17 Which of the following pH values indicate a neutral solution? (1 point)* O pH=2 O pH=5 O pH=7 OpH=9 Question 18 Which of the following forms a solution with a pH of 13.7? (1 point) O 0.02M solution of NaOH O 0.04M solution of Mg(OH)2 0.2M solution of HCI 0.5M solution of NaOH
7) Which of the following forms a solution with a pH of 1.7? (a) 0.02M solution of HCl (b) 0.02M solution of NaOH (c) 0.5M solution of HCl (d) 0.8M solution of HNO3 8) What is the pH of a 0.0045 M HBr solution? (a) 11.65 (b) 13.2 (c) 2.35 (d) 7.05 9) What is the pOH of a 0.0045 M HBr solution? (a) 11.65 (b) 13.2 (c) 2.35 (d) 7.05
Question 20 Which of the following forms a solution with a pH of 1.7? (1 point)* 0.02M solution of HCI O 0.02M solution of NaOH 0.5M solution of HCI O 0.8M solution of HNO3 Question 21 Which of the following represents a conjugate acid-base pair? (1 point) All of the above CH3COOH / CH3COO- CH3COOH/COO CH3COOH/NH3
In which of the following titrations would the solution be neutral at the equivalence point? Select one: a. NH3 titrated with HCl b. Sr(OH)2 titrated with H3PO4 c. HOCl titrated with Ba(OH)2 d. CH3COOH titrated with NaOH e. HClO4 titrated with KOH
Mixing 0.02M HCl 100ml with 0.20M CH3COOH (Ka=1.8*10^-5) 100ml obtained a 200ml solution. Which choose the correct alternative. a) [H+]=0.11M b) [H+]=0.01M c) [CH3COO-]=1.34*10^-3M d) [Cl-]=0.2M
When 1 Liter volumes of the below solutions are mixed, which will result in the precipitation of PbCl2? (Ksp = 1.7 * 10^-5) a.) 0.04M Pb(NO3)2 and 0.08M KCl b.) 0.001M Pb(NO3)2 and 0.05M KCl c.) 0.002M Pb(NO3)2 and 0.02M KCl d.) 0.01M Pb(NO3)2 and 0.005M KCl
In which of the following titrations would the solution be neutral at the equivalence point? [Hint: For a neutral equivalence point, we need both a strong acid and a strong base as analyte and titrant, respectively.] HOCl titrated with Ba(OH)2 CH3COOH titrated with NaOH HClO4 titrated with KOH Sr(OH)2 titrated with H3PO4 NH3 titrated with HCl
MY UTEP Dashb... ou (Open Learning) 5 Physio EX 9.1 Cengage/ MindTap Question 20 Which of the following forms a solution with a pH of 1.7? (1 point) O 0.02M solution of HCI 0.02M solution of NaOH O 0.5M solution of HCI 0.8M solution of HNO3