Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- True or false? A titrant for an acid-base titration analysis must be chosen to have an endpoint (change of colour) at very nearly the same pH as the equivalence point pH of the reaction solution.arrow_forwardThe primary buffer in the blood is carbonate-bicarbonate buffer. If the pKa is 6.1 and the pH is set at 7.4, what is the ratio of the concentrations of carbonate to bicarbonate. Describe the buffering capacity of this buffer.arrow_forward5) Determine the ratio in which sodium acetate and acetic acid must be mixed to give a solution that is buffered at pH 6.500.arrow_forward
- What effect has a 1:10 times dilution of a buffer solution with pure water on its useful range or its buffer capacity?arrow_forwardThe weak base NH3 (concentration 0,10 mol∙dm–3) is titrated with strong acid HCl (concentration 0,050 mol∙dm–3). Without doing any calculations, explain why the pH at the equivalence point of this titration is less than 7.arrow_forwardDetermine the pH of a buffer solution that is a mixture containing 0.10M acetic acid and 0.050 M sodium acetate, provided that the Ka of acetic acid is 1.8 x 10-5.arrow_forward
- if the change in pH after addition of 1.0mL of 0.10N HCI is 0.09, what is the total buffer capacity of the 20mL solution?arrow_forwardUse the following experimental titration data to calculate the concentration of the acid being analysed. Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade.arrow_forwardUsing the Henderson-Hasselbalch equation, demonstrate that the pH at 50% neutralisation for a monoprotic acid/base titration is equal to the pKa for the acid.arrow_forward
- Explain why 6M NH3 and not 6M NaOH solution is used when separation Fe3+ and Al3+ ions from Ca2+, Cu2+, and K+ ions in the qualitative analysis of cations. Write appropriate chemical equations to support your conclusion.arrow_forwardLakes have a natural buffering capacity, especially in regions where limestone gives rise to dissolved calcium carbonate. Write an equation for the effect of a small amount of acid rain containing sulfuric acid if it falls into alake containing carbonate (CO3-2 ) ions. Discuss how the lake will resist further pH changes. What happens if a large excess of acid rain is deposited?arrow_forwardDiscuss the titration curve (variation of pH with respect to addition oftitrant) with suitable diagram and reactions involved when potassiumhydroxide (KOH) a strong base is added as titrant to acetic acid(CH3COOH) a weak acid analyte.arrow_forward
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