7. Ammonium hydroxide is a weak base because Group of answer choices it is only slightly soluble in water it dissociates only slightly in water. it is completely ionized in aqueous solution. it is a dilute solution it cannot hold on to its hydroxide ions     8. The Ka for hydrofluoric acid is 7.2 × 10-4.  This means that HF is   Group of answer choices able to react with HCl a strong acid ionic neutral in water solution. a weak acid.

Determining how many protons (H* ions) an acid can donate and a base can accept is an important aspect in acid/base reactions. The lemon and lime juices you will be using in Parts B and C of this experiment contain citric acid, which is a triprotic acid. Knowing that citric acid is a triprotic acid, how will it stoichiometrically react (what ratio, acid:base) with the standardized NaOH solution that will be used as the titrant? O 3:1 O 2:1 O 1:2 O 1:3

A solution has [H3O+] = 4.4×10−5 M . Use the ion product constant of water Kw=[H3O+][OH−] to find the [OH−] of the solution.   A solution has [OH−] = 2.5×10−2 M . Use the ion product constant of wate Kw=[H3O+][OH−] to find the [H3O+] of the solution.

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A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? pH B. What is the hydroxide ion concentration, [OH], in an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A-(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.190 M, [H*] = 4.00 x 104 M, and [A-] = 4.00 x 104 M. Calculate the Ką value for the acid HA. Ka = TOOLS x10"

Explain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H,CO, and a salt of its conjugate base NaHCO3 O Excess acid is removed by reacting with NaHCO3; excess base is removed by reacting with H,O O Excess base is removed by reacting with NaHCO3; excess acid is removed by reacting with H2CO3 O Excess H,O is removed by reacting with NaHCO3; excess base is removed by reacting with H,CO

4. Which of the following statements is true? A) In an acidic solution, the concentration of OH is less than H₂O In a basic solution, the concentration of OH is less than H,0 C) In a basic solution, the concentration of OH' is equal to H,O D) In an acidic solution, the concentration of H,O' is less than OH

What is the resulting pH of a solution that forms when 20.00 mL of a 0.150 mol/L hydrochloric acid solution combined with 12.50 mL of a 0.200 mol/L sodium hydroxide solution? greater than 7 less than 7 equal to 7 O The solution will not have a pH. The pH must be determined experimentally.

1. A solution of Ba(OH)2 has a [OH-] of 0.40 M. What is the initial molar concentration of the solution? 2. A solution of LiOH has a pH of 13.68. What is the initial concentration of the solution. 3. A solution of Hbr has a [OH-]= 5.0 x 10-12 M. What is the pH of the solution? 4. The [OH-] of CsOH is 0.025 M. What is the pH of the solution? 5. What is the initial concentration of a solution of CsOH with a ph=13.68? 6. A solution of HCl has a pOH=12.08. What is the initial concentration of the solution? 7. The Ka of acetic acid is 1.8x10-5 at 25 degrees C. What is the pH of 0.25 M CH3COOH? 8. The Kb of ammonia is 1.8 x 10-5 at 25 degrees C. What is the pH of 0.25 M NH3?