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I would need help with these questions step by step:
- Calculate the isoelectric and isoionic pH of 0.010 M threonine? pK1 = 2.15, pK2 = 9.12
- Find the pH of a 1.00 L aqueous solution containing 12.43 g of tris (FM 121.14) plus 4.67 g of tris hydrochloride ( FM 157.60) ? What would be the new pH after adding 12.0 mL of 1.00 M NaOH to this buffer?
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- I would need help with these problems, please show step by step: 1. A beaker containing 500.0 mL was determined to contain 0.150 M ammonia (NH3) and 0.150 M ammonium chloride NH4 To this solution was added 50.0 mL of 0.15 M hydrochloric acid (HCl). What was the change in pH of the ammonia, ammonium ion solution? 2. Calculate the isoelectric and isoionic pH of 0.010 M threonine? pK1 = 2.15, pK2 = 9.12 3. Find the pH of a 1.00 L aqueous solution containing 12.43 g of tris (FM 121.14) plus 4.67 g of tris hydrochloride ( FM 157.60) ? What would be the new pH after adding 12.0 mL of 1.00 M NaOH to this buffer?There are many organic acids and bases in our cells, and their presence modifies the pH of the fluids inside them. It is useful to be able to assess the pH of solutions of acids and bases and to make inferences from measured values of the pH. A solution of equal concentrations of lactic acid and sodium lactate was found to have pH= 3.08. (a) What are the values of pKa and Ka of lactic acid? (b) What would the pH be if the acid had twice the concentration of the salt?A group of wealthy chemistry 1A students had a little too much disposableincome and decided to create the most expensive they could think of. Using various spectroscopictechniques the salt was determined to be rhodium (III) Bromide (RhBr3). When this salt was shaken withpure water at 25°C, the solubility was found to be 0.026 mg/mL. Calculate the Ksp of RhBr3
- Calculate Qsp for calcium fluoride (Ksp = 3.9 ×10–11) when 180.0 mL of a 7.95×10-3 M solution of Ca(NO3)2 is added to 310.0 mL of a 6.90×10-3 M solution of KF.A sample of anhydrous NaHCO3 (FM = 84.007) is suspected to be contaminated with either NaOH (FM = 39.997) or Na2CO3 (FM = 105.989). To verify the suspicion, a 0.7483 g sample was dissolved to prepare a 50.00 mL solution, and a 10.00 mL aliquot was taken to prepare a 100 mL solution, where 25.00 mL was analyzed using double flask method. If the sample requires 0.45 mL of standard 0.0125 N HCl to reach the phenolphthalein endpoint and 35.95 mL to reach the bromcresol green endpoint, calculate the percentage composition (in %w/w) of all the basic components in the sample.A sample of anhydrous NaHCO3 (FM = 84.007) is suspected to be contaminated with eitherNaOH (FM = 39.997) or Na2CO3 (FM = 105.989). To verify the suspicion, a 0.7483 g sample was dissolved to prepare a 50.00 mL solution, and a 10.00 mL aliquot was taken to prepare a 100 mL solution, where 25.00 mL was analyzed using double flask method. If the sample requires 0.45 mL of standard 0.0125 N HCl to reach the phenolphthalein endpoint and 35.95 mL to reach the bromcresol green endpoint, calculate the percentage composition (in %w/w) of all the basic components in the sample.
- In the preparation of the standard curve for protein analysis, 50 mn BSA (bovine serum albumin) dissolved in H2O to a final volume of 5 mL was used as stock solution. What is the weight of BSA in 0.1 mL of stock solution? In 0.2 mL?Given a solution of 0.0025 M HC2H3O2, Ka = 1.8 x 10^-5 a. Calculate the pH of the solution. b. Calculate pKa. c. Calculate the Kb value for C2H3O2-.If the concentration of an acid in solution is 2.2 times larger than the concentration of its conjugate base, and the pH of the solution is 3.5, what is the pKa of the acid? Include the answer to 3 significant figures
- In which of the following mixture(s) would CaF2(s) (Ksp = 4.0 x 10-11) form? 30 mL of 0.00020 M Ca(NO3)2 + 20 mL of 0.00125 M NaF 20 mL of 0.00020 M Ca(NO3)2 + 30 mL of 0.00125 M NaF 10 mL of 0.00020 M Ca(NO3)2 + 40 mL of 0.00125 M NaF Group of answer choices I only II only I and II I and IIIThe ethyl mercaptan (C2H5SH, 62.13 g/mol) concentration in a mixture was determined by shaking a 1.534 g sample with 50.0 mL of 0.01293 M I2 in a tightly stoppered flask: 2 C2H5SH (aq) + I2 (aq) --> C4H10S2 (aq) + 2 I- (aq) + 2 H+ (aq) The excess I2 was back-titrated with 15.72 mL of 0.01425 M Na2S2O3: I2 (aq) + 2 S2O32- (aq) --> 2 I- (aq) + S4O62- (aq) Calculate the percentage of ethyl mercaptan in the sample (3 sf)Use the Goal Seek spreadsheet at the end of the chapter to find the pH of 1.00 L of solution containing 0.030 mol HA (pKa = 2.50) and 0.015 mol NaA. What would the pH be with the approximations [HA] = 0.030 and [A-] = 0.015?