A 10 mL volume of a 5 mM lactic acid solution is mixed with 5 mL of water. What is the concentration of the resulting mixture in
To calculate this problem, consider the serial dilution formula: Molarity (start) x Volume (start) = Molarity (final) x Volume (final) or M1V1 = M2V2.
Thus, 5×10 = ?× 15 = 3.3 mM
Convert the millmolar into micromolar gives 3300 µM, hence the concentration of the resulting mixture is 3.3 ×103 µM.
Need help on Problem 7 & 8 Vi CI 7. A 10 mL volume of a 5 mM lactic acid solution is mixed with 5 mL of water. What is the concentration of the resulting mixture in uM? (Remember, CV,=C2V2, where C and V represent the concentrations and volumes of each solution, respectively.) Finaca C2 5avi = Cava (5x10-3) Clomi) = (Ca)(151) 15ml 15ml 8. What volume of water should be added to 7 mL of a 10 mM riboflavin...
Equal volumes of 200 mM lactic acid and 200 mM potassium lactate are mixed to make a buffer. The pKa of lactic acid is 3.86 (a) Determine the pH of this buffer and its final concentration. [4 marks] (b) Calculate the concentrations of the buffer components after acid or base is added to bring the pH to 4.5. Assume a negligible change in volume. 6 marks]
10 ml containing 1.0 mmole of lactic acid solution, CH3CH(OH)COOH, (pKa=3.86) was titrated with NaOH solution up to a total volume of 100 ml a. what is the concentration of the base solution required for a full neutralization of the lactic acid? b. what is the pH at the equivalent point? c. what will be the pH of the solution obtained after adding 0.2 mmole of NaOH(S) (SOLID!)
1. What volume of 0.10 M NaOH is needed to neutralize 100 mL of 0.050 M HCl? 2a. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.01 M of HNO3 solution, what is the concentration of H+ and the pH in the resulting mixture? 2b. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.02 M of HCl solution, what is the concentration of H+ and the pH in...
A 7.00 mL aliquote of acetic acid was mixed with water and the resulting solution was titrated with 0.250 M NaOH. It took 40.2 mL of base to reach the equivalence point. What was the concentration of the acetic acid? 1) 0.043 M 2) 0.070 M 3) 0.143 M 4) 1.43 M
10) 2.00 mL ofa 0.0500 M CusO, solution is mixed with 2.00 mL of a 0.0100 M solution of K. Ksp (CuF2) 1.61 x 109 a) (7 pts) What is the concentration of Cu (aq) ion in the solution after equilibrium is established? b) (6 pts) Water is added to bring the volume of the solution to 1.00 L, and the mixture is stirred until equilibrium is reestablished. Calculate Q for this mixture. Is all of the CuF2 dissolved?
If you mix 200. ml of a 0.150 M solution of lactic acid with 0.010 moles of solid Ba(OH)2, what is the pH of the resulting solution? You may neglect the volume change from the Ba(OH)2 addition.
2)250.0 mL of a 0.375 M solution of lactic acid (HC:H:03) is titrated with a solution of 0.75 M NaOH. The K, for lactic acid is 1.38 x 104. (22 pts total) a) what is the pH before addition of NaOH? (Hint: what is the relevant equilibrium?) (4 pts) b) what is the total number of moles of acid? (2 pts) c) what volume of the NaOH solution is required to reach the equivalence point? (2 pts) d) what is...
1) A 20.0 mL sample of lactic acid (monoprotic with Ka = 1.37 x 10-4) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution? 1.0.120 M 2. 0.200 M 3. 0.300 M 4. 6.00 x 10-3 M 5. cannot be found without the molar mass of lactic acid. 2) Oxalic acid is diprotic with pKa1 = 1.23 and pKa2 = 4.19. What is pKb for the hydrogen...
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