1) Which of the following solutions will have the highest pH? and Why? A. 0.20 M...

Question

Question

1) Which of the following solutions will have the highest pH? and Why?

A. 0.20 M HCl
B. 0.20 M HNO3
C. 0.20 M HBr
D. 0.20 M HC2H3O2

2) The enthalpy of which of the following reactions is equivalent to the hydrogen-fluorine (H-F) bond energy?

A. 2 HF (g) →H2(g) + F2(g)
B. ½ H2(g) + ½ F2(g) →HF (g)
C. HF (g) →H (g) + F (g)
D. H (g) + F (g) →HF (g)

science chemistry

Answer 1

Similar Homework Help Questions

Which of the following 0.10 M aqueous solutions gives the highest pH? A) CH3COOH (pKa =...

Which of the following 0.10 M aqueous solutions gives the highest pH? A) CH3COOH (pKa = 4.75) B) HF (PK:= 3.45) C) H3PO4 (pKal = 2.12) D) HCIQ (Ka=2.00) E) Since all are acids, the pH is the same for all solutions. 5. Which one of the following salts gives an acidic aqueous solution? A) CsNO3 B) CaCl2C ) LiF D) Cr(CIO4)3 E) NaCH3CO2 6. 7. All of the following are strong acids except A) HCIQB) HC104 C) HI D)...
Order the following three solutions from smallest to largest pH: 0.20 M HClO3 0.0030 M HNO3...

Order the following three solutions from smallest to largest pH: 0.20 M HClO3 0.0030 M HNO3 1.50 M HCl
The pH of two separate solutions, 1.0 M HNO3 and 1.0M HC H302, are measured. Which...

The pH of two separate solutions, 1.0 M HNO3 and 1.0M HC H302, are measured. Which statement is true? The HNO3 has a higher pH because it is a strong acid. The HC2H302 has a higher pH because it is a weak acid, The HC2H302 has a higher pH because it has more acidic hydrogen atoms. The HC H30, has a lower pH because it has more acidic hydrogen atoms. The two solutions have the same pH because the concentrations...

Which one of the following aqueous solutions will have a pH of 0.00 at 25 °C?...

Which one of the following aqueous solutions will have a pH of 0.00 at 25 °C? (Kw = 1.0 ´ 10–14) 0.10 M HNO3 1.0 M NaOH 1.0 * 10^1 M HBr 1.0 M KCl 1.0 M HCl
What is the pH value of the following composition of solutions? a) 1 mL 0.10 M...

What is the pH value of the following composition of solutions? a) 1 mL 0.10 M HC2H3O2 + 99 mL H2O b) 5 mL 0.10 M HC2H3O2 + 5 mL 0.10 M HCl c) 0.10 M H3PO4 d) 0.10 M NH3 e) 0.10 M NH4NO3 f) 50 mL 0.10 M NH3 + 50 mL 0.10 M NH4NO3 g) 10 mL Solution (h) + 6 mL H2O h) 10 mL Solution (h) + 5 mL H2O + 1 mL 0.10 M...
Calculate the pH of each of the following strong acid solutions. (a) 0.00851 M HCl pH...

Calculate the pH of each of the following strong acid solutions. (a) 0.00851 M HCl pH = (b) 0.714 g of HNO3 in 18.0 L of solution pH = (c) 62.0 mL of 4.90 M HCl diluted to 3.00 L pH = (d) a mixture formed by adding 55.0 mL of 0.00326 M HCl to 46.0 mL of 0.00896 M HNO3 pH =

Calculate the pH of each of the following strong acid solutions. (a) 0.00757 M HBr pH...

Calculate the pH of each of the following strong acid solutions. (a) 0.00757 M HBr pH = (b) 0.264 g of HCl in 16.0 L of solution pH = (c) 60.0 mL of 6.70 M HBr diluted to 4.50 L pH = (d) a mixture formed by adding 80.0 mL of 0.00838 M HBr to 80.0 mL of 0.00258 M HCl pH =
Calculate the pH of the following solutions (show your work) (a) 0.018 M of HBr (b)...

Calculate the pH of the following solutions (show your work) (a) 0.018 M of HBr (b) 0.115 M of HF (Ka = 3.5 * 10^-4) (c) 0.015 M of HI mixed w/ 0.02 M of HNO3
Find the pH of each of the following solutions of mixtures of acids. No Ka is...

Find the pH of each of the following solutions of mixtures of acids. No Ka is given. Part A.) 0.125 M in HBr and 0.145 M in HCHO2 (Gave up, Answer pH= 0.903) Part B.) 0.145 M in HNO2 and 9.0×10−2 M in HNO3 Part C.) 0.190 M in HCHO2 and 0.23 M in HC2H3O2

Arrange the following 0.10 M solutions in order of decreasing pH (highest to lowest): NaCIO, KCI,...

Arrange the following 0.10 M solutions in order of decreasing pH (highest to lowest): NaCIO, KCI, HBr, NaBro, CH3NH3Br NaBro > NaCIO > KCI > CH,NH,Br > HB Nacio > CH,NH3Br > NaBro > KCI > HBr CH, NH,Br > NaBrO > Nacio > KCI > HBO Nacio > NaBro > KCI > CH,NH,Br > HBO NaBro > CH NH,Br > NaCIO > KCI > HBO Arrange the following reactions in order of increasing tendency to proceed to completion (least...