Would the following solutions provide an effective buffer. a) 250. mL of 0.15 M HC2H3O2 + 25 mL of 0.10 M NaOH yes no b) 125 mL of 0.50 M HNO2 + 75 mL of 0.40 M KNO2 yes no c) 250. mL of 0.25 M HCO2H + 125 mL of 0.50 M KOH yes no d) 250. mL of 0.50 M HClO4 + 150. mL of 0.50 M NaClO4 yes no e) 250. mL of 0.50 NaOH + 500. mL of 0.50 M NH4NO3 yes n
Would the following solutions provide an effective buffer. a) 250. mL of 0.15 M HC2H3O2 +...
Which of the following solutions will produce a buffer solution? 0.50 M KOH/0.50 M KCI 0.50 M HF/0.50 M HC2H302 0.50 M NH3/0.50 M KF 0.50 M HCIO4/0.50 M NaClO4 0.50 M NH3/0.50 M NH4NO3
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCI must be added to this buffer solution to change the pH by 0.40 units? Assume the total volume remains unchanged at 400 mL. For H2PO4, K = 6.3 x 10-8 0.013 mol 0.25 mol (Your answer) 0.50 mol 0.057 mol (Correct answer) 0.031 mol
What is the pH value of the following composition of solutions? a) 1 mL 0.10 M HC2H3O2 + 99 mL H2O b) 5 mL 0.10 M HC2H3O2 + 5 mL 0.10 M HCl c) 0.10 M H3PO4 d) 0.10 M NH3 e) 0.10 M NH4NO3 f) 50 mL 0.10 M NH3 + 50 mL 0.10 M NH4NO3 g) 10 mL Solution (h) + 6 mL H2O h) 10 mL Solution (h) + 5 mL H2O + 1 mL 0.10 M...
Which of the following solutions would have the lowest buffer capacity? 0.10 M H2CO3, 0.15 M NaHCO3 2.0 MHC2H302, 2.0 M KC2H302 1.0 M HCOOH, 1.15 M NaHCOO 0.50 MH3PO4, 0.35 M KH2PO4
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
Which solutions below would be described as a buffer solution? A) 500 mL of 0.1 M HCl added to 500 mL of 0.1 M NaOH B) 500 mL of 0.1 M HCl added to 500 mL of 0.1 M NaCl C) 500 mL of 0.1 M HCNO added to 500 mL of 0.1 M KCNO D) 500 mL of 0.1 M HCNO added to 250 mL of 0.1 M KCNO E) 500 mL of 0.1 M HCNO added to 250...
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
Given 100. mL of each of the three aqueous buffer solutions: Buffer A is 0.50 M in ammonia and 0.10 M in ammonium chloride; Buffer B is 0.50 M in ammonia and 0.50 M in ammonium chloride; and Buffer C is 0.50 M in ammonia and 1.0 M in ammonium chloride. To each of the 100. mL samples is added 1.0 mL of 6.0 M hydrochloric acid. Which buffer solution will show the smallest change in pH? Explain why.
4. What is the pH of a 100.0 mL buffer solution containing 0.15 M NaHCO3 and 0.15 M Na2CO3? 5. What is the pH after adding 15.0 mL of 0.10 M NaOH to the solution in question 4?
5. Calculate the pH of the following solutions. (4 pts) 0S18 500257 a) 0.25 M NHCI solution b) 0.10 M NaHCO3 solution 6. b) A student mixes 8.203 g of NaC2H3O2 with 100 mL of 1.0 M HC2H3O2, what is the pH of the buffer? (4 pts) b) If you add 5.0 mL of 0.5 M NaOH solution to 20.0 mL to the buffer above, what is the pH of the resulting solution? (4 pts)