A buffer contains significant amounts of ammonia and ammonium chloride. (Part A) Enter an equation showing how this buffer neutralizes added aqueous acid (HNO3). Express your answer as a chemical equation. Identify all of the phases in your answer. (Part B) Enter an equation showing how this buffer neutralizes added aqueous base (NaOH). Express your answer as a chemical equation. Identify all of the phases in your answer. ** Make sure to identify ALL phases (states) in your answer **
1. Part.A
A buffer is any type of substance that will resist pH change when H+ or OH- is added.
When a weak acid and its conjugate base are added, they will form a buffer
The equations:
For the weak base equilibrium:
B(aq) + H2O(l) <------------> BH+(aq) + OH-(aq)
Weak base = B;
Conjugate acid = BH+
Neutralization of OH- ions:
BH+(aq) + OH-(aq) <-------> B(aq) + H2O(l); in this case, OH- is neutralized by BH+, as well as B is created
Neutralization of H+ ions:
B(aq) + H+(aq) <--------> BH+(aq)
So, Equation showing how this buffer neutralizes added HNO3 is
NH4OH (aq) + HNO3 (aq) -----------> H2O (l)+ NH4NO3 (aq)
Part.B
Equation showing how this buffer neutralizes added base (NaOH) is :
NH4Cl (aq) + NaOH (aq) ------------> NH3 (aq) + NaCl (aq) + H2O (l)
A buffer contains significant amounts of ammonia and ammonium chloride. (Part A) Enter an equation showing...
A buffer contains significant amounts of ammonia and ammonium chloride. Part A: Enter a net ionic equation showing how this buffer neutralizes added aqueous acid (HI). Express your answer as a chemical equation. Identify all of the phases in your answer. Part B: Enter a net ionic equation showing how this buffer neutralizes added aqueous base (CsOH). Express your answer as a chemical equation. Identify all of the phases in your answer.
3. A buffer contains significant amounts of ammonia and ammonium chloride. Write equations to show how this buffer neutralizes added acid and added base. Include one sentence of explanation for each equation.
Part A Write an equation that shows how this buffer neutralizes added acid. Express your answer as a chemical equation. Identify all of the phases in your answer.Part B Write an equation that shows how this buffer neutralizes added base. Express your answer as a chemical equation. Identify all of the phases in your answer.
A buffer contains significant amounts of acetic acid and sodium acetate. Write an equation showing how this buffer neutralizes added acid (HNO3 (aq). Write an equation showing how this buffer neutralizes added base (KOH(aq)).
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
1. Write a chemical equation for NaOH(aq) showing how it is an acid or a base according to the Arrhenius definition. Express your answer as a chemical equation. Identify all of the phases in your answer. 2. Write a chemical equation for H2SO4(aq) showing how it is an acid or a base according to the Arrhenius definition. Express your answer as a chemical equation. Identify all of the phases in your answer. 3. Write a chemical equation for HBr(aq) showing...
(UNITS_26_27 Exercise 17.34 - Enhanced - with Feedback A buffer contains significant amounts of ammonia and ammonium chloride.
A 1.0 L buffer solution contains 0.74 moles of ammonia 0.74 moles of ammonium chloride. Kb = 1.8 x 10—5 . Calculate the pH of this buffer after the addition of 0.10 moles of NaOH.
A buffer solution contains 0.392 M ammonium chloride and 0.498 M ammonia. If 0.0206 moles of perchloric acid are added to 150 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding perchloric acid)
A buffer solution contains 0.322 M ammonium chloride and 0.486 M ammonia. If 0.0545 moles of hydrochloric acid are added to 250 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding hydrochloric acid.)