A solution of 5 x 10-3 M MnO4- is dissolved in 25.00 mL of H2O. What volume of H2O must be added to the solution to reduce the concentration of [MnO4- ] to 7.5 x 10-4 M?
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A solution of 5 x 10-3 M MnO4- is dissolved in 25.00 mL of H2O. What...
5 H2O2 + 2 MnO4- +6 H+502 +8 H2O +2 Mn2+ 3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration?
What volume of 0.0850 M HCl is required to titrate 25.00 mL of a 0.100 M NH3 solution to the equivalence point?? Please show work so I can understand -- thank you.
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6 H...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6H→ 5...
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...
Prepare 25.00 mL of solution which is 0.60M in isopropanol (0.785 g/mL) and 1.00 M in HCL. What volume (in mL) of isopropanol will you need to add in part II of the experiment? Also, if a reaction is is second order with respect to isopropanol concentration (and I'm assuming that that would mean the plot of 1/[MnO4 ^2-] vs time is the most linear), what will happen to the rate when you halve the concentration of isopropanol? It would...
A 25.00 mL sample of an unknown sulfuric acid solution is titrated with 29.84 mL of a sodium hydroxide solution with a concentration of 0.150 M NaOH. What is the concentration of the sulfuric acid solution? H.SO.(aq) + 2NaOH(aq) → Na2SO4 (aq) + 2 H2O(1) Show your work Final Answer
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH with 25.00 mL of 0.050 M CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 x 10-5 for CH3COOH.
The following table shows the data for the titration of 25.00 mL of 0.200 M CH3COOH (pKa= 4.75) with 0.200 M NaOH (sodium hydroxide). Volume of NaOH added (mL) pH of the solution (measured) Mols of CH3COO-formed Mols CH3COOH remained pH of the solution (calculated) 0.00 2.72 0 0.005 2.70 10.00 4.57 0.002 0.003 4.57 12.50 4.7 0.0025 0.0025 4.75 24.90 7.14 0.0049 2 x 10-5 7.14 24.99 8.14 0.00 2 x 10-6 8.15 25.00 8.88 0.005 0 8.88 25.01...
The actual concentration was found to be 0.002364 M. 4. Knowing that 1 mole of dissolved oxygen ends up reacting with 4 moles of the titrant S2032, how do you calculate the amount of dissolved oxygen (in units of mg/L) from the volume of titrant added? Show your work. (2.5 pts) • Use X (mL) as your total volume of titrant added. • Use the actual concentration of the -0.0025 M NazS2O3 solution used during the titration (calculated in question...