NH3 is a weak base (Kb = in NH4Cl at 25 °C? pH = x10 TOOLS 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.046 M

NH3 is a weak base ( ?b=1.8×10−5 ) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.019 M NH4Cl at 25 °C?

Caluculate the pH and percent ionization of a 0.20 M CH;NH2 solution. (K, = 5.6 × 104)

An aqueous solution of a monoprotic acid HA (Ka = 3.03x 10^-1) has a pH of 4.10. What is the molarity of the solution? (i.e. [HA] + [A-].)

What is the pH of a 0.0380 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

Sulfuric acid is a diprotic acid.    It's a two stages of ionization as shown below.               H2SO4  (aq)  →→  H+   + HSO4- (aq)    pKa  =  ???              HSO4- (aq)   ↔↔ H+    +  SO42-   pka  =  1.991                          a)   Calculate the concentration of HSO4-   &  SO42-  ion in a 0.5000 M  H2SO4 solution.            b)    Determine the pH of the solution to the correct number of significant figures. Q1A:   3.95 g NH4HCO3 is added to  1000 ml of water, What are the H3O+, OH-, NH3, and HCO3-?

What is the pH of the solution that results from adding 24.7 mL of 0.11 M HCl to 25.2 mL of 0.41 M NH3 ? (K, for ammonium ion is 5.6 x 10-10 ) pH =

What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.220 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 × 10⁻⁴)

HCIO is a weak acid (K₁ = 4.0 × 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a solution that is 0.064 M in NaCIO at 25 °C? pH =

For the diprotic weak acid H2A, Kal = 2.5 × 10-6 and K2 = 6.5 x 10-9. What is the pH of a 0.0400 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A?- in this solution? [H, A] = [A?-] =