A laboratory technician needs to make a
8181-liter
batch of a
2020%
acid solution. How can the laboratory technician combine a batch of an acid solution that is pure acid with another that is
1010%
to get the desired concentration?
The laboratory technician can combine
. 9.9
L of the pure acid solution with
80.180.1
L of the
1010%
acid solution to get the desired concentration.
A laboratory technician needs to make a 8181-liter batch of a 2020% acid solution. How can...
7. A laboratory needs to find out the concentration of a solution of nitrous acid (HNO2, a monoprotic acid). The laboratory technician uses a procedure just like you will use in this laboratory activity. In Part l, the technician titrates the barium hydroxide solution against a standard, solid acid. It is found that the barium hydroxide solution is 0.198 M in barium hydroxide In Part Il, the technician places a 25.00 ml sample of the nitrous acid solution in an...
A chemist needs to mix an 18% acid solution with a 45% acid solution to obtain a 12 liter mixture consisting of 36% acid. How many liters of each acid solutions must be used?
A 100 mL solution needs to have a concentration of 36.50 mg/mL of pure Sodium Salicylate. Using a batch of sodium salicylate with a 95.5% assay, how many grams (g) of sodium salicylate do you need to achieve the desired concentration for a 100 mL solition?
Mike needs to make 2 liters of a 0.3 M NaOHsolution for an experiment. He has a 1.2 M stock solution. How much stock solution must he dilute to reach his desired 2 liter, 0.3 M final solution? Select the correct answer below: 0.18 L 0.5 L 1.2 L 8.0 L
You wish to make a 0.249 M hydrobromic acid solution from a stock solution of 12.0 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? __mL You wish to make a 0.112 M nitric acid solution from a stock solution of 12.0 M nitric acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution? __mL In the...
A student needs to make a buffer solution with a pH of 5.08 using acetic acid and sodium hydroxide starting with 100.0 mL of 0.38 M acetic acid. Calculate the number of moles of sodium hydroxide that should be added to achieve the desired pH.
number 23 acid buffer described in Problem 21, you discover that your m ion? laboratory is out of sodium acetate, but you do have sodium hydroxide. How much (in moles and grams) acetic acid and til the pH on of the sodium hydroxide do you need to make the buffer? f th ola . Another alternative. Your friend from another labora- ory was out of acetic acid, so tries to prepare the buffer in Problem 21 by dissolving 41.02 g...
1. In the laboratory, a student dilutes 27.6 mL of a 10.2 M hydrobromic acid solution to a total volume of 150.0 mL. What is the concentration of the diluted solution? Concentration = ______M How many milliliters of 11.8 M hydrobromic acid solution should be used to prepare 2.50 L of 0.400 M HBr? ______mL 2. In the laboratory a student combines 41.2 mL of a 0.440 M cobalt(II) acetate solution with 23.1 mL of a 0.311 M lead acetate...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need...
A chemist needs to make a buffer solution with a pH of 4.25 with a solution that currently contains 465 mL of 0.0941 M NaOH. The chemist plans to use acetic acid as the weak acid in the buffer. a) what should be the molar ratio of conjugate base to weak acid in the buffer solution? b) how many moles of acetic acid would need to be added to neutralize all of the sodium hydroxide? c) how many moles of...