1. Consult an appropriate source and determine the Concentration of each of the following species, when...
1. Consult an appropriate source and determine the Concentration of each of the following species, when in Concentrated form: HCl, H2SO4, and NH3.
2. A 10mL solution of 0.010M HCl is mixed with 20mL of a 0.01M Pb2+ solution, giving a total volume of 30mL. What are the concentrations of Cland Pb2+ after the mixing? Will a precipitate of PbCl2 form? (Ksp = 1.7 x 10-5 for PbCl2 at 25oC.)
3. In the Group 2 precipitations, the Sulfide Ion (S2- ) is generated in an Acidic environment. If the H2S concentration is maintained at 0.1M and the pH = 1, what is the [S2- ] concentration? (Ka1 = 1 x 10-7 and Ka2 = 1 x 10-13 for H2S.)
4. In the Group 3 precipitations, the pH is raised by adding Ammonia. Suppose it is raised to pH = 9. What is the [S2- ] concentration under these conditions? Assume the H2S concentration is again 0.1M.
Homework Answers
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1. Consult an appropriate source and determine the Concentration
of each of the following species, when...
In the Group 3 precipitations, the pH is raised by adding Ammonia. Suppose it is raised...
In the Group 3 precipitations, the pH is raised by adding Ammonia. Suppose it is raised to pH = 9. What is the [S2- ] concentration under these conditions? Assume the H2S concentration is again 0.1M. Consult an appropriate source and determine the Concentration of each of the following species, when in Concentrated form: HCl, H2SO4, and NH3.
a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid...
a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid if the pH of this is 4.18. Ka1 (H2CO3) =4.45 x 10–7 and Ka2 =4.69 x 10–11 (b) Calculate the pH at the equivalence point of the titration between 0.1M CH3COOH (25 ml) with 0.05 M NaOH. Ka (CH3COOH) = 1.8 x 10–5.
Find the pH of each solution: 1. 30mL of 0.1M K2HPO4 mixed with 10mL of 0.1M...
Find the pH of each solution: 1. 30mL of 0.1M K2HPO4 mixed with 10mL of 0.1M KH2PO4 and 60mL of water; 2. 10mL of 0.1M K2HPO4 mixed with 30mL of 0.1M KH2PO4 and 60mL of water; Phosphoric acid, H3PO4 1st Ka&pKa 7.1 x 10-3 2.15 2nd Ka&pKa 6.3 x 10-8 7.20 3rd Ka&pKa 4.5 x 10-13 12.35
Calculate the sodium acetate molar concentration of each dilution. Record the calculated values in Data Table...
Calculate the sodium acetate molar concentration of each dilution. Record the calculated values in Data Table 2. The concentration of the 4.7 pH buffer is 0.05 M sodium acetate. Concentration(start) x Volume(start) = Concentration(final) x Volume(final) pH 4.7 buffer (10 mL sodium acetate, 10 mL water) 1st dilution (5 mL pH 4.7 buffer solution, 15 mL water) 2nd dilution (5mL of 1st dilution, 15mL water) 3rd dilution (5mL of 2nd dilution, 15mL water) Calculation Help 5mL if 0.1M sodium acetate...
1. Using the given information answer the following questions with corresponding answers. (a) Tryptophan is a...
1. Using the given information answer the following questions with corresponding answers. (a) Tryptophan is a diprotic acid (Ka1 = 1.48 × 10-3 and Ka2 = 4.07 × 10-10) that can have three different form in solution: H2T+, HT, and T-. What would be the pH of the solution containing 0.045M HT? Group of answer choices 6.86 6.12 7.43 12.23 7.06 (b) Tryptophan is a diprotic acid (Ka1 = 1.48 × 10-3 and Ka2 = 4.07 × 10-10) that can...
1. Using the given information answer the following questions with corresponding answers. (a) Serine is a diprotic acid...
1. Using the given information answer the following questions with corresponding answers. (a) Serine is a diprotic acid (Ka1 = 6.17 × 10-3 and Ka2 = 7.08 × 10-10) that can have three different forms in solution: H2S+, HS, and S- (Note: S is not sulfur in these formulas). What would be the concentration of H2S+ in the solution of 0.105M Na+S-? Group of answer choices 8.29 × 10-8 M 1.62 × 10-12 M 9.62 × 10-9 M 4.15 ×...
1. A comic book villain is holding you at gun point and is making you drink...
1. A comic book villain is holding you at gun point and is making you drink a sample of acid. She gives you a beaker with 100ml of a strong acid with pH=5. She also gives you a beaker of a strong base with a pH=10. You can add as much of the strong base to the strong acid as you want, and you must then drink the solution. You'd be best off trying to make the solution neutral before...
1 A) Which of the following pairs of solutions when mixed will form a buffer solution?...
1 A) Which of the following pairs of solutions when mixed will form a buffer solution? Group of answer choices H2SO4 and Ca(OH)2 NH3 and NH4Br NaNO3 and HNO3 KOH and KNO2 B)Phosphoric acid, H3PO4, is a triprotic acid with the following Ka values: Ka1 = 7.5 x 10-3; Ka2 = 6.2 x 10-8; Ka3 = 3.6 x 10-13 In a solution of 0.15 M H3PO4, which species will be most abundant? H3O+ H3PO4 HPO42- H2PO4-
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a...
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a 0.123 M solution of the weak acid, sulfurous acid (H2SO3). The stepwise dissociation constants of carbonic acid are: Ka1 1.41 x 102 Ka2-6.31 x 108 3. Consider the following dissociation of the triprotic acid, phosphoric acid (HsPOs): Step 1 H3POa + H2O <=> H30+ + H2PO4, Step 2 HP0i + H2O <=> H30+ + HP042- Step 3 HPO42-+ H2O <-> H3O+ + PO43- Kal=7.1...
1. A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is...
1. A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid? 2. A weak monoprotic acid has pKa = 3.08. Calculate the percent ionization of a 0.35 M solution of this acid. 3. Calculate the pH of a solution that is 0.050 M in CH3COOH...
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a 0.123 M solution of the weak acid, sulfurous acid (H2SO3). The stepwise dissociation constants of carbonic acid are: Ka1 1.41 x 102 Ka2-6.31 x 108 3. Consider the following dissociation of the triprotic acid, phosphoric acid (HsPOs): Step 1 H3POa + H2O <=> H30+ + H2PO4, Step 2 HP0i + H2O <=> H30+ + HP042- Step 3 HPO42-+ H2O <-> H3O+ + PO43- Kal=7.1...
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