Select all examples of abiotic factors.

Answer the following question.  Submit your final answer here. A 25.00 mL aliquot of the weak  (HA) acid was titrated with 0.1185 M NaOH(aq) using both an indicator and a pH meter. Ka (HA), is 6.50 x10-4. A total of 29.38 mL of 0.1185 M NaOH(aq)  was required to reach the equivalence point. 1. Calculate the molarity of the acid solution. (4 pts) 2. Calculate the pH of the  acid solution before titration (Hint: use the RICE table). (4 pts) 3. Calculate the pH and [A-] at the half-equivalence point. (3 pts) 4. Calculate the pH at the equivalence point of the titration. (Hint: use Kb for hydrolysis of A- anion and RICE table). (3 pts) 5. Suggest an appropriate indicator for titration. Explain your choice. (2 pts) 6. Calculate the pH of the solution after 20.00 mL of 0.1185 M NaOH(aq) was added. (Hint: ignore the spectator sodium ion and find moles of acid and A- and use Henderson-Hasselbalch equation). (2EC) To receive full credit, show all work in handwriting or use the software showing calculations and units properly and clearly. Indicator pKa Phenolphthalein 9.3 Bromothymol blue 7.0 Methyl red 5.0 Thymol blue 2.0 Methyl violet 0.80 GL

Answer the following question.  Submit your final answer here. Write the balanced equation and use a correct mole ratio to calculate how many milliliters of 0.01154 M HCl are required to titrate 20.00 mL of 0.0125M Ca(OH)2?

Answer the following question.  Submit your final answer here. Calculate the pH of the solution obtained by mixing 48.00 mL of 0.1110M NaOH and 52.00 mL of 0.0995M HCl

Answer the following question.  Submit your final answer here. Use the Henderson-Hasselbalch equation to calculate the pH of the solution prepared by dissolving  0.55 mol of a weak acid (Ka=2.77×10-5) and 0.78 mol of its conjugate base in enough water to make 1.00L of buffer solution

Answer the following question.  Submit your final answer here. The molar solubility of the salt with generic formula A2B is 1.07 × 10-7 M in pure water.  Calculate the Ksp for this salt.

Answer the following question.  Submit your final answer here. Write the balanced equation and use a correct mole ratio to calculate how many milliliters of 0.1154 M NaOH are required to titrate 10.00 mL of 0.0950M H2SO4 to the second equivalence point?

Answer the following question.  Submit your final answer here. Consider a saturated Me(OH)2 solution. Ksp for Me(OH)2= 2.08 × 10-15 Calculate the molar solubility of Me(OH)2 in pure water. (7 pts) Calculate the molar solubility of Me(OH)2 in 0.95M Me(NO3)2. (4 pts) Compare the molar solubility of Me(OH)2 in pure water and in the buffer solution with pH 6. Justify your answer. (1) After submitting the exam, upload the matching calculations to the Exam 3 Solutions, Extra Credit, and Partial Credit assignment. Answers – 3pts, work – 1pts

An investor holds two independent assets. Over the next year the dollar profit from asset 1 is and from asset 2 is , both in thousands of dollars. Let be the portfolio’s total profit. Using the empirical rule (about 68% of a normal distribution lies within one standard deviation of the mean), what is the approximate probability that total profit exceeds $63,000, i.e. ? Give your answer to two decimal places. (Hint: what are the mean and variance of ?)

The daily output (in tons) of a small workshop is a continuous random variable with density and otherwise. What is the variance of daily output, ?