Question

In: Chemistry

1. Calculate the hydronium ion concentration and pH for a 0.042 M solution of sodium formate,...

1. Calculate the hydronium ion concentration and pH for a 0.042 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11.

[H3O+]----------------M

pH---------------------

2.

What are the equilibrium concentrations of NH3, NH4+, and OH- in a 0.42 M solution of ammonia? What is the pH of the solution?

Kb = 1.8 * 10^-5

[OH-] ----------------------- M

[NH4+] ----------------------M

[NH3] ---------------------- M

pH----------------------------

Solutions

Expert Solution


Related Solutions

Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2....
Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11. [H3O+] =_____ M pH =______
What is the hydronium ion concentration in a 0.0294 M aqueous solution of sodium arsenate (Na3AsO4)?
What is the hydronium ion concentration in a 0.0294 M aqueous solution of sodium arsenate (Na3AsO4)?
Part A: Calculate the pH of a solution that is 0.250 M in sodium formate (HCOONa)...
Part A: Calculate the pH of a solution that is 0.250 M in sodium formate (HCOONa) and 0.110 M in formic acid (HCOOH). Part B: Calculate the pH of a solution that is 0.520 M in pyridine (C5H5N) and 0.470 M in pyridinium chloride (C5H5NHCl). Part C: Calculate the pH of a solution that is made by combining 55 mL of 0.040 M hydrofluoric acid with 125 mL of 0.120 M sodium fluoride.
Calculate the hydronium ion concentration and the pH when 65.0 mL of 0.45 M NH3 is...
Calculate the hydronium ion concentration and the pH when 65.0 mL of 0.45 M NH3 is mixed with 65.0 mL of 0.45 M HCl (Ka = 5.6x10^-10). Concentration = pH=
A. Calculate the hydronium ion concentration in an aqueous solution of 0.185 M carbonic acid, H2CO3...
A. Calculate the hydronium ion concentration in an aqueous solution of 0.185 M carbonic acid, H2CO3 (aq) B. Calculate the concentration of HCO3- in an aqueous solution of 0.1860 M carbonic acid, H2CO3 (aq).
The hydronium ion concentration of a pH neutral aqueous solution is decreased by three orders of...
The hydronium ion concentration of a pH neutral aqueous solution is decreased by three orders of magnitude. Is it acidic or basic? pH increase or decrease? By how many pH units does the pH change? Does the molar concentration of hydroxide increase or decrease? By how many orders of magnitude does the molar concentration of hydroxide change?
Calculate the hydronium ion concentration and the pH when 50.0ml of 0.40M NH3 is mixed with...
Calculate the hydronium ion concentration and the pH when 50.0ml of 0.40M NH3 is mixed with 50.0ml of 0.40M Hcl
Calculate the values of the hydroxide ion concentration, pOH, and pH for a 0.20 M solution...
Calculate the values of the hydroxide ion concentration, pOH, and pH for a 0.20 M solution of ammonia
The hydronium ion concentration of an aqueous solution of 0.530 M hydroxylamine (a weak base with...
The hydronium ion concentration of an aqueous solution of 0.530 M hydroxylamine (a weak base with the formula NH2OH) is ... [H3O+] = ____M
The hydronium ion concentration of an aqueous solution of 0.546 M triethylamine (a weak base with...
The hydronium ion concentration of an aqueous solution of 0.546 M triethylamine (a weak base with the formula (C2H5)3N) is ..
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT