Which of the following compounds could be used to create a buffer with a pH of 9.00? ammonia, Kb = 1.76 x 10–5 None of the above compounds could be used to create a buffer with a pH of 9.00. p-toluidine, pKb = 8.92 formic acid, Ka = 1.80 x 10–4 benzene-1,2,3-tricarboxylic acid, pKa1=2.88, pKa276, pKa3 = 7.13
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- ammonia, Kb = 1.76 x 10–5
- None of the above compounds could be used to create a buffer with a pH of 9.00.
- p-toluidine, pKb = 8.92
- formic acid, Ka = 1.80 x 10–4
- benzene-1,2,3-tricarboxylic acid, pKa1=2.88, pKa276, pKa3 = 7.13
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- Which of the following buffer solutions containing CH3COONa and CH3COOH would have a pH of 4.88? Ka for CH3COOH is 1.8 x 10–5. Which of the following buffer solutions containing CH3COONa and CH3COOH would have a pH of 4.88? Ka for CH3COOH is 1.8 x 10–5. 1. 0.055 M CH3COONa and 0.015 M CH3COOH 2. 0.055 M CH3COONa and 0.055 M CH3COOH 3. 0.075 M CH3COONa and 0.055 M CH3COOH 4. 0.015 M CH3COONa and 0.055 M CH3COOH 5. 0.015 M CH3COONa and 0.075 M CH3COOHWhat will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?After a buffer solution of carbonic acid (with pKa of 3.75) was added with 1ml of sulfuric acid, the resulting pH of the carbonic acid buffer solution is 1.25. Do you think the carbonic buffer system still works effectively after the addition of the said acid?
- What is the pH of a buffer that is 0.120 M in chloroacetic acid(ClC2H3O2H) and 0.800 M in potassium chloroacetate (KClC2H3O2)? For chloroacetic acid, Ka = 1.4 x 10-4.A buffer solution consists of 0,25 mol∙dm–3 acetic acid (HC2H3O2; Ka= 1,8 x 10–5) and 0,35 mol∙dm–3 potassium acetate (KC2H3O2). Calculate the pH of the buffer solution. A small quantity (0,050 mol) of solid KOH is added to 1 dm3 of the buffer. This quantity is so small that it does not affect the volume of the buffer. Calculate the new pH of the buffer solution after the KOH has been added.gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.(a) BaSeO4, 0.0118 g/100 mL(b) Ba(BrO3)2∙H2O, 0.30 g/100 mL(c) NH4MgAsO4∙6H2O, 0.038 g/100 mL(d) La2(MoO4)3, 0.00179 g/100 mL
- What are the pKa values and buffering capacity of these following buffer components? Ammonium/Ammonia buffer Lactic acid/Lactate buffer Phosphoric acid/hydrogen PO4 buffer Benzoic acid/Benzoate bufferWhich conjugate acid/base pair could be used to create a pH 3.20 buffer solution with the largest possible buffer capacity? Sulfurous acid/sodium bisulfite Hydrofluoric acid/sodium fluoride Nitrous acid/sodium nitrite Benzoic acid/sodium benzoate Acetic acid/sodium acetate pKa=1.92 pKa=3.14 pKa=3.34 pKa=4.20 pKa=4.74Write the equilibrium-constant expression Kc for Cd2+(aq) + 4 Br-(aq) => [CdBr4]2-(aq).
- Which of the following acids (listed with pKa values) and their conjugate base should be used to form a buffer with a pH of 8.10? HC7H5O2, pKa = 4.19 HF, pKa = 3.46 HClO, pKa = 7.54 H2SO3, pKa = 1.77 HClO2, pKa = 1.96A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00 mL of water and is titrated with 0.1086 M NaOH. What is the expected pH during this analysis when the titration is complete?calculate the ph of a 0.465 M solUTION OF ethylamine CH3CH2NH2 and 0.211 M ethylammonium bromide CH3CH2NB3Br. the base dissociation constant kb is 6.31 x 10 -4. what is the pH if 76.0 ml of 0.150 M of a strong acid like HCI is added to 100 ml of buffer solution. what if a strong base like NaOh is added with the same ammount instead