A 100 mL solution of 0.10 M weak base NH3 (Kb = 1.8 10-5) is titrated with 1.0 M strong acid titrant HCl. NH3 + H2O → NH4+ + OH- A.What is the acid and base pH before titration? B. How much acid is required to achieve the equivalence point and the midway point where pH = pKa? C. Write your own titration curve,include pH after 50 mL of acid is added, at the equivalence point, and after 60 mL of acid is added.

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Q: base?                           Is the unknown solution strong or weak?…

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Q: 6. For the following acid -base titration H2SO4 (aq) + NaOH(aq) ----> A. Write down a complete and…

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Q: a. How many grams of dry NH4CI need to be added to 2.40 L of a 0.300 M solution of ammonia, NH3, to…

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Q: 13. Consider a 50 mL solution of 0.150 MNH3 (Kb = 1.8 x 10-5). You are titrating it with a solution…

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Q: Write a balanced chemical equation for the neutralization reaction of (a) hydrochloric acid and (b)…

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Q: The pH at the equivalence point for the titration of a weak acid with a strong base will always be O…

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Q: 1. Consider the titration of 50.0 mL of 0.100 M HA (a weak acid with K.-4.0 x 10) with 0.100 M KOH.…

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Q: Weak base with strong acid Practice: titration of 25.00 ml of 0.10 M NH3 with 0.10 M HCl at 25 °C.…

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Q: 5 mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia…

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Q: a. What is the pH of a buffer solution that is 0.28 M NH3 and 0.28 M NH4+? K for NH3 is 1.8 × 10-5…

A: Given :  a.  Concentration of NH3 = 0.28 M  Concentration of NH4+ = 0.28 M  Kb of NH3 = 1.8 x 10-5…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.