A 100. ml sample of 0.10 M HCl is mixed with 50. ml of 0.10 M...

A 100. ml sample of 0.10 M HCl is mixed with 50. ml of 0.10 M NH₃. What is the resulting pH?

Thank you!

Expert Solution

no of moles of HCl = molarity * volume in L

= 0.1*0.1 = 0.01 moles

no of moles of NH3 = 0.1*0.05 = 0.005moles

HCl + NH3 ---------> NH4Cl

I 0.01 0.005 0

c -0.005 -0.005 0.005

E 0.005 0 0.005

[H+] = no of moles of Hcl at equilibrium /total volume in L

= 0.005/0.15 = 0.0333M

PH = -log[H+]

= -log0.0333 = 1.4775

queen_honey_blossom answered 2 years ago

A 168.5 mL sample of 0.087 M HCl is mixed with 50.2 mL of 0.089 M...

A 168.5 mL sample of 0.087 M HCl is mixed with 50.2 mL of 0.089 M NH3. What is the resulting pH? (The Kb for NH3 = 1.8 x 10^5).

A 100 mL solution of .400 M Sodium Acetate (NaOAc) mixed with 100 ml of .400 M HCl.

Determine the [H3O+] and [OH-] for the following: A 100 mL solution of .400 M Sodium Acetate (NaOAc) mixed with 100 ml of .400 M HCl.

Sketch a titration curve for 50 mL of 0.10 M HCl titrated with 0.15 M NaOH....

Sketch a titration curve for 50 mL of 0.10 M HCl titrated with 0.15 M NaOH. Include on the graph: a) The initial pH b) The volume of the equivalence point c) The pH at the equivalence point d) The pH after addition of 50 mL of NaOH SHOW STEPS

28 mL of 0.10 M HCl is added to 60 mL of 0.10 M Sr(OH)2. Using...

28 mL of 0.10 M HCl is added to 60 mL of 0.10 M Sr(OH)2. Using proper unit cancellation, determine the concentration of OH− in the resulting solution.

3. A 30.0-mL sample of 0.10 M C2H3NH2 (ethylamine) is titrated with 0.15 M HCl. What...

3. A 30.0-mL sample of 0.10 M C2H3NH2 (ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 20.00 mL of acid have been added to the amine? Kb = 6.5 × 10–4

230 mL of 0.10 M NaOH are added to 100 mL of 0.10 M H3PO4. What...

230 mL of 0.10 M NaOH are added to 100 mL of 0.10 M H3PO4. What is the pH of the resulting solution?

Consider the following four titrations. i. 100.0 mL of 0.10 M HCl titrated by 0.10 M...

Consider the following four titrations. i. 100.0 mL of 0.10 M HCl titrated by 0.10 M NaOH ii. 100.0 mL of 0.10 M NaOH titrated by 0.10 M HCl iii. 100.0 mL of 0.10 M CH3NH2 titrated by 0.10 M HCl iv. 100.0 mL of 0.10 M HF titrated by 0.10 M NaOH Rank the titrations in order of: increasing volume of titrant added to reach the equiva- lence point. increasing pH initially before any titrant has been added. increasing...

250. mL of 0.600 M HCl is mixed with 250. mL of 0.600 M NaOH ,...

250. mL of 0.600 M HCl is mixed with 250. mL of 0.600 M NaOH , resulting in a neutralization reaction with net ionic equation: H+ (aq) + OH- (aq) → H2O(ℓ) ∆Hrxn = -57.0 kJ Assume the solutions have specific heat capacity of 4.18 J/g C , and the solutions have a density of 1.00 g/mL. The reaction takes place in a coffee-cup calorimeter, and all heat transfer occurs within the confines of the calorimeter. If the initial temperature...

If 85.00 mL of 0.100 M HCl is mixed with 25.00 mL of 0.200 M H2SO4...

If 85.00 mL of 0.100 M HCl is mixed with 25.00 mL of 0.200 M H2SO4 and 50.00 mL of 0.400 M NaOH. What is the resulting pH of the final solution? Please show all work and how the formulas are derived if modified.

50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate...

50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate the following: a. The solubility of Ag2CrO4 (Ksp = 1.9 X 10-12) in the solution in moles per liter. b. The concentrations of the following ions Ag+, CrO4-2, K+, and NO3-.

Question