A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph above. What is a pH value between 2.5- 7.5 where the concentration of the weak acid being titrated is less than the concentration of its conjugate base?

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A: Given:Volume of HCl (V1) =20.00 mL =0.020 LMolarity of KOH (M2) = 1.70 x 10-4 MVolume of KOH (V2) =…

Q: Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution…

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Q: NaOH(aq) + HCI(aq) → NaCl(s) + H2O(aq) Calculate the pH of the solution that results from the…

A: Millimoles of NaOH reacted = 404 x 4.88 x 10-5 = 0.0197 millimoles Millimoles of HCl reacted = 566 x…

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Q: was performed as follows: 10.00 mL of 0.10M HCl were collected in an Erlenmeyer flask, and then…

A: D option is correct. pH = 2.15 so, nearly solution is 2.11.

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Q: Cu2+(aq) + H2O(l) ⇌ CuOH+(aq) + H+(aq)   Keq = 1.2 x 10−8 A 1.00 M solution of copper(II) nitrate…

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Q: HCN(aq)+H2O(l) ⇄ H3O+(aq)+CN−(aq)               Ka=[H3O+][CN−] / [HCN]=6.2×10−10 The equilibrium…

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Q: many mL of 0.2016 M KOH would be expected to be used in the titration of 0.3266 g of a diprotic acid…

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Q: What would be the hydronium ion concentration in a solution 0.100 M NaOH and 1.00 M NH3? (Hint:…

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Q: By titration, it is found that 50.1 mL of 0.192 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Given, Molarity of NaOH = 0.192 M Volume of NaOH = 50.1 ml Volume of HCl = 25.0 ml  Molarity of HCl…

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.