Concept explainers
(a)
Interpretation:
If the given statement is true or false needs to be determined.
The given net ionic equation shows the tiration of NaF versus
Concept introduction:
Titration is to determine the quantitative information of the unknown sample when a known volume and concentration of reactant is utilized. It is usually an acid-base reaction. The unknown solution is the titrantand the known volume of solution is the titrant.
(b)
Interpretation:
If the given statement is true or false needs to be determined.
The given reaction is a reaction between a strong acid and base.
Concept introduction:
Titration is to determine the quantitative information of the unknown sample when a known volume and concentration of reactant is utilized. It is usually an acid-base
(c)
Interpretation:
If the given statement is true or false should be determined.
The solution acts as buffer at equivalnce point.
Concept introduction:
Titration is to determine the quantitative information of the unknown sample when a known volume and concentration of reactant is utilized. It is usually an acid-base reaction. The unknown solution is the titrantand the known volume of solution is the titrant. At the equivalence point, the color of the indicator changes.
(d)
Interpretation:
If the given statement is true or false should be determined.
The pH of the solution is not changed if the solution at half-neutralizartion is diluted with water.
Concept introduction:
Titration is to determine the quantitative information of the unknown sample when a known volume and concentration of reactant is utilized. It is usually an acid-base reaction. The unknown solution is the titrantand the known volume of solution is the titrant. At the equivalence point, the color of the indicator changes.
(e)
Interpretation:
If the given statement is true or false should be determined.
For the given case, phenolphthalein is a good indicator to be used.
Concept introduction:
Titration is to determine the quantitative information of the unknown sample when a known volume and concentration of reactant is utilized. It is usually an acid-base reaction. The unknown solution is the titrantand the known volume of solution is the titrant. At the equivalence point, the color of the indicator changes.
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Check out a sample textbook solutionChapter 14 Solutions
Chemistry: Principles and Reactions
- When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.arrow_forwardWrite the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forwardGiven three acid-base indicators—methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)—which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acidarrow_forward
- Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.arrow_forwardWhich compound in each pair is more soluble in water than is predicted by a calculation from Ksp? (a) AgI or Ag2CO3 (b) PbCO3 or PbCl2 (c) AgCl or AgCNarrow_forwardWhen a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If the pH at 50.0 mL NaOH added is 4.0, and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka1, and Ka2 for the diprotic acid.arrow_forward
- Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.arrow_forwardThe buffer capacity indicates how much OH- or H+ ions a buffer can react with. What is the buffer capacity of the buffers in Problem 10?arrow_forwardA student makes a buffer from 100 mL of 0.10 M formic acid (HCOOH) and 100 mL of 0.10 M potassium formate (KCHOO). Upon addition of 20 mL of 1M NaOH solution, the student observes the pH is significantly higher than the original pH of the buffer, and concludes the buffer was defective. Is the student correct? What is the buffer capacity?arrow_forward
- A titration experiment is set up where 41.84 mL of 0.4334 M ethylamine, C2H5NH2, is titrated using 1.3218 M HNO3 (the HNO3 is placed in the burette). What should be the pH of the titration reaction after 37.54 mL of HNO3 is added?arrow_forwardConsider exactly one litre of a hydrofluoric acid buffer solution, containing 0.800 M HF and 0.528 M F-1. Determine the pH of the buffer solution.- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations- Ka for hydrofluoric acid is 6.6 × 10−42. Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 × 10−2 M HCℓ solution is added to it. You must indicate all the relevant reaction equations in your working.arrow_forwardYou have two different concentrations of a buffer solution, 2.0 M and 0.20 M, to which 0.01 mol HCl has been added. Which of these solutions has the higher buffer capacity? In other words, which would be able to resist pH via the addition of acid longer?arrow_forward
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