5.4 A buffer contains 0.1076 mol NH3 (Kb =1.8 x10-5) and 0.1193 mol of NHẠNO3 in a 355 mL solution. Determine the pH of the buffer after addition of 0.0050 mol Ba(OH)2 solution. (Assume that the change in volume on the addition of Ba(OH)2 is negligible.) QUESTION 6: ELECTROCHEMIS TRY
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- What happens when too much NaSCN is prepared in solution of mixtures of standard solutions of Fe(NO3)3 and NaSCN, so that [SCN^-] is higher than expected? What does this do to the measured Keq?10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8, respectively. Which one would be more suitable for use in asolution buffered at pH = 7.0? What other substances would be needed to makethe buffer?
- 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?30mL 0.9% v/v green food coloring. Transfer 2mL of of food coloring to flask, QS the flask to 100mL with DI water. What is the concentration of the standard?For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surely
- A mixture of NaBr, Nal and NaNO3 weighs 0.6500 g. With AgNO3, a precipitate of the two halides is obtained and is found to weigh 0.9390 g. When heated in a current of C2, the precipitate is converted entirely to AgCi weighing 0.6566 g. What is the %NaNO3 in the original sample?In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid ( 1mL ≎0.0031g Na2O) What is the normality of NaOH?A 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is pQsp for A3D4?
- The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 * 10-4 and 3.0 * 10-8, respectively. Which one would be more suitable for use in a solution buffered at pH = 7.0? What other substances would be needed to make the buffer?The following text may be found at the ThermoFisher website: "PBS (phosphate buffered saline) is a pH-adjusted blend of ultrapure-grade phosphate buffers and saline solutions which, when diluted to a 1X working concentration, contains 137 mM NaCl, 2.7 mM KCl, 8 mM Na2HPO4, and 2 mM KH2PO4. Each 10X PBS solution is ready to use upon dilution to the desired concentration." This means that the product that you purchase has a concentration 10 times the concentration at which it is used. 1. Look up the pKa values for phosphoric acid and list them as a part of your response. 2. Based on the description of the contents of the PBS buffer, calculate the pH of the 1X solution. 3. Assume that you wish to use a pH = 7.00 buffer. If your answer to 2 was more acidic than pH 7.00, calculate how much 1.00 M NaOH you would need to add to get to pH = 7.00. If your answer to 2 was more basic than pH 7.00, calculate how much 1.00 M HCl you would need to add to get to pH = 7.00.A 50-mL solution of 0.5005 N standard NaOH was added to a 0.9250-g sample of Aspirin and was boiled for 10 minutes. After cooling a full pipet of phenolphthalein was added to the solution before it was titrated with 24.7 mL of 0.5015 N standard HCl solution until the disappearance of the pink color. The same procedure was carried using a blank which consumed 4.6 mL of the same standard acid. Calculate for the %Aspirin in the sample. Atom weights: C =12, H =1, O =16.