pH = 10.31 Use the following table to predict the best acid/ base pair for the desired pH/pOH values below (hint: remember buffer range = ± 1 pKa unit). Acid Base     Name Acid Base pKa Hydrochloric acid HCl Cl- -7.00 Phosphoric acid H3PO4 H2PO4- 2.12 Hydrofluoric acid HF F- 3.18 Lactic acid Lactic acid Lactate 3.85 Acetic acid CH3COOH CH3COO- 4.74 Carbonic acid H2CO3 HCO3- 6.36 Dihydrogen phosphate H2PO4- HPO42- 7.21 Ammonium NH4+ NH3 9.25 Hydrocyanic acid HCN CN- 9.31 Bicarbonate HCO3- CO32- 10.25 Methylammonium ion CH3NH3+ CH3NH2 10.62 Hydrogen phosphate HPO42- PO43- 12.38

Again consider the same buffer solution from the previous question, where [H2CO3] = [HCO3–] = 0.100 M. What will be the pH after 0.005 mol of NaOH has been added to 1.00 L of this solution? (Ka1 for H2CO3 = 4.2 x 10–7) Group of answer choices

What are the answers to the following questions.

Complete the following table. Be sure to show each calculation in detail.

We want to prepare a buffered solution having a pH of 4.97 using concentrated (23.6 M) formic acid (HCOOH) and solid sodium formate (HCOONA). Ką for formic acid is 1.8 x 10-4. Incorrect. Calculate the ratio [HCOO (aq)] / [HCOOH(aq)] in the buffered solution required to achieve a pH of 4.97. [HCOO (aq)] /[HCOOH(aq)] = i 1.68E1 eTextbook and Media Hint Save for Later Attempts: 2 of 3 used Submit Answer

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Calculate the concentrations of the weak acid and conjugate base for the best possible buffer at pH 3.50 knowing that the concentration of the more concentrated species between the two will be 0.2 M. Choose the buffer system you think would be best between the following three. You will need to look up literature values for the Ka/pKa on your own. Remember that a strong buffer has similar concentrations of the buffering components. Formic acid/formate Acetic acid/acetate Hypobromous acid/Hypobromite

If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.270 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.45.                H2CO3(aq)  ⇌  HCO3-(aq) + H+(aq)                                 Ka = 5.3 × 10-7 Show all calculations including equation(s) used. Provide your final answer to 3 decimal places.

= O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: name acetic acid hypochlorous acid solution 0.1 M NACIO 0.1 M C5H5NHCI acid 0.1 M NaNO3 0.1 M KCH3CO₂ 0 Explanation formula HCH3CO₂ 1.8 x 10 -5 HCIO Check 3.0 × 10 pH ✓choose one 1 (lowest) 2 Ka 3 4 (highest) choose one X-5 choose one ◊ 7 0 -8 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. ? base K₂ formula pyridine CHN 1.7 x 107 -9 ammonia name + A ALEKS-... NH3 NH3 AN 30 1.8 × 10 -5 tv h MacBook Air Þ G 0/5 Hannah S Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center AO Accessib

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