Questions 26-29 refer to the same strong acid/strong base (SA/SB) titration. Prior to the beginning of the titration, there were 0.0050 moles of HI present in the flask. (Q27) A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH when 30.00 mL of titrant have been added?
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- Questions 26-29 refer to the same strong acid/strong base (SA/SB) titration. Prior to the beginning of the titration, there were 0.0050 moles of HI present in the flask. (Q26) A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the initial solution pH (when 0.00 mL of titrant have been added)Questions 30-35 refer to the same weak acid/strong base (WA/SB) titration. Prior to the beginning of the titration, there were 0.0090 moles of hypobromous acid present in the flask. The Ką of hypobromous acid is 2.8 x 10-9. (Q30) A 30.00 mL solution of 0.300 M hypobromous acid (HBRO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LIOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)?Questions 26-29 refer to the same strong acid/strong base (SA/SB) titration. Prior to the beginning of the titration, there were 0.0050 moles of HI present in the flask. (Q28) A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH at the equivalence point?
- 5. 25.00 mL of HCN (K₂=4.90 x 10-10) was titrated with 18.50 mL of 0.0125 M Ca(OH)2. a) What is the concentration of HCN in the original sample? b) What is the pH after 9.25 mL of base have been added? c) What is the pH of the solution at the endpoint of the titration?Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K of pyridine is 1.7 x 10-⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution when 15.00 mL of titrant have been added? (Two decimal places) Type your answer...Consider the titration of 60.0 mL of 0.0400 M H₂NNH₂ (a weak base; Kb = 1.30e-06) with 0.100 M HI. Calculate the pH after the following volumes of titrant have been added: (1) 24.0 mL (2) 45.6 mL pH = pH =
- (5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]Questions 40-45 refer to the same weak base/strong acid (WB/SA) titration. Prior to the beginning of the titration, there were 0.0280 moles of pyridine present. The Kp of pyridine is 1.7 x 10-9. (Q42) A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution when 15.00 mL of titrant have been added?Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH,);N (K, = 5.2 x 10-4), with 0.1000 M HCl solution after the following additions of titrant. (a) 13.00 mL: pH = 10.305 (b) 20.10 mL: pH = (c) 29.00 mL: pH = %3!
- Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H20 S H;0* + In¯ Using the results from the experiment, identify which of the reactant/product are responsible for the red and green color of the indicator. Notes: solution turns red after adding acid; solution turns blue/green after adding base RED: BLUE/GREEN: Why is the color violet/blue at pH near 7? Answer in 1 sentence. Hint: What is the relationship of the species responsible for the observed colors?In the titration of 50.0 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10−5) with 0.100 M NaOH calculate the pH when: (8 pts) 0 mL of NaOH is added 0 mL of NaOH is added 0 mL of NaOH is added 0 mL of NaOH is added12 pH 7- a ml added 1. The titration curve represents the titration of (a) strong acid titrates a strong base. (b) strong acid titrates a weak base. (c) strong base titrates a weak acid. (d) weak acid titrates a weak base. 2. Using the chart of indicators (below), select a suitable indicator for the end point of the titration. pH Range 3.1 – 4.4 Indicator (a) Methyl orange (b) Bromothymol blue (c) Thymol blue (d) Cresol red 6.0 – 7.6 1.2 – 2.8 7.2 – 8.8