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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:Consider the titration of 80.0 mL of 0.100 M Ba (OH), by 0.400M HCl. Calculate the pH of the resulting solution after the following volumes of HCI have been added.
a. 0.0 ml
pH =
Ь. 20.0 mL
pH =
c. 30.0 mL
pH =
d. 40.0 mL
pH =
e. 90.0 mL
pH =
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- Consider a solution that contains 0.50 moles of HF and 0.50 moles of NaF in 1.0 L of water. If 0.15 mol of HCI is added to this buffer solution, the pH of the solution will get slightly The pH does not change more drastically because the HNO3 reacts with the present in the buffer system.arrow_forwardConsider the titration of the 25.0 mL 0.125 M weak base (monobasic) with 0.0625 M HCl. Calculate the following. Determinethe pH when 90.0 mL of the titrant has been added (answer in two decimal places) =arrow_forwardAn aqueous solution contains 0.30 M ammonium bromide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.14 mol HCI O0.30 mol HCI O0.07 mol Ba(OH)2 0.29 mol NH3 0.29 mol CaBr2arrow_forward
- The pH of a bicarbonate-carbonic acid buffer is 5.63. Calculate the ratio of the concentration of carbonic acid (H₂CO3) to that of the bicarbonate ion (HCO3). Be sure your answer has the correct number of significant digits. Note: Reference the pK, of acids at 25 °C table for additional information. [HCO3] [H₂CO3]]arrow_forwardConsider the following titration curve of a weak base titrated with a strong acid. How would the pH be calculated at point 1 on the curve? 14 1 12 2. 10 3 4 10 20 30 40 30 60 HCl added (mL) O By subtracting the mol of weak base initially present from the mol of strong acid added to calculate the molarity of strong acid O As a weak acid equilibrium using the K, and the concentration of acid added O As a weak base equilibrium using the Ki and the concentration of base initially present As a buffer using using the K, and the ratio of weak base to conjugate acid Hdarrow_forwardCalculate pH for a weak acid/strong base titration. Determine the pH during the titration of 64.2 mL of 0.368 M hypochlorous acid 3.5x10-8) by 0.368 M NaOH at the following points. (Ka (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 96.3 mL of NaOHarrow_forward
- A buffer solution contains 0.235 M ammonium bromide and 0.314 M ammonia. If 0.0164 moles of hydrobromic acid are added to 125 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume change does not change upon adding hydrobromic acid) pH =arrow_forward200.0 mL of an acetate/acetic acid buffer is .100 M in total molarity and has a pH of 5.000. After 6.30 mL of 0.490 M HCl is added, what is the new pH?arrow_forwarda buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…arrow_forward
- I don’t know how to do this questionarrow_forwardHow many moles of potassium hydroxide would have to be added to 250 mL of a 0.385 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.360? molesarrow_forwardDetermine the pH during the titration of 21.9 mL of 0.277 M perchloric acid by 0.206 M sodium hydroxide at the following points: (1) Before the addition of any sodium hydroxide (2) After the addition of 14.8 mL of sodium hydroxide (3) At the equivalence point (4) After adding 35.4 mL of sodium hydroxidearrow_forward
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