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What is the pH of a 0.0200 M Na3PO4 solution, show hydolysis equation and ICE table. If 5% assumption is used, verify x.
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How was x calculated, was quadratic or the 5% assumption used?
- Cr2O7 2- (aq) + 14H+ 6e- ---> Cr3+(aq) + 7H2O(l) Ered = 1.33V Cu2+(aq) + 2e- --> Cu(s) ?°red = 0.34V Determine the Ecell at 25°C, given: [Cr2O7(aq) 2- ] = 0.2500M ,[Cr(aq) 3+ ] = 0.2500M , pH =5 [Cu2+]=0.2500MFull acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.MATLAB The acidity of solutions is generally measured in terms of pH. The pH of a solution is defined as theconcentration of hydronium ions. Create a table of conversions from concentration of hydronium ionto pH, spaced logarithmically from 0.001 to 0.1 mol/liter with 10 values. Assuming that you havenamed the concentration of hydronium ions H_conc, the syntax for calculating the negative of thelogarithm of the concentration (and thus the pH) is:pH = -log10 (H_conc)
- Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1) find Ka and use the value of Ka to calculate the initial pH of each trial 2) calculate Kb for the C8H4O4^-2 anion from the value of Ka that you obtained for KHP.If pH (± 0.5 pH units) strips were used to determine the equivalence point at pH=8.5. What is the relative error (%) in pH at the equivalence point? I assumed it should be 0.5/8.5 * 100 = 5.88, rounded to 5.9 for sig figs. but I got the answer wrong. Please help and let me know how to solve this.
- please give calculation as well. Calculate the pH value of each of the solutions in tubes 1-9 using the Henderson-Hasselbalch equation (H-H eqn).Determine the pl of casein. Compare your experimental values with those found in the literature. Biomolecules. Thank you! The protein is casein.Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.A 0.1 M solution of acid was used to titrate 10 ml of 0.1 M solution of alkali and thefollowing volumes of acid were recorded: 9.88 10.18 10.23 10.39 10.21 Calculate the 95% confidence limits of the mean and use them to decide whetherthere is any evidence of systematic error.
- MUST ANSWER BOYH SUBPARTS A AND B A 1.161g sample of pure maleic acid (H2M, 116.1 g/mol) with Ka1 and Ka2 values of 1.42 × 10-2 and 8.57 ×10-7, respectively, was contained in a 100.0 mL solution with a pH of 5.0. In solution, maleic acid can dissociate into HM- and M2- species. The three species (H2M, HM- and M2-) exist in the solution at varying concentrations that depend on the pH of the solution. a) Calculate the values of α1 (alpha 1) and α3 (alpha 3). b) Calculate the concentration of HM- in the above solution.The pH of a saturated soloution of magnesium hydroxide, Mg(OH)2, (milk of magnesia) was found to be (1.080x10^1). From this, find the Ksp for magnesium hydroxide. Express your answer to three significant figures. Note: Your answer is assumed to be reduced to the highest power possible.I did an experiment: Molar concentration of Fe (NO3)3=.002 Molar concentration of NaSCN= .002 On my 1st trial: Volume of Fe(NO3)3 = 5 mL Moles of Fe3+, initial (mol) = 1 x 10-5 Volume of NaSCN (mL)= 1 mL Moles of SCN-,initial (mol)= 2 x 10-6 Absorbance was .08 Now trying to find Calculation of Kc I already found [FeNCS2+] equilibrium, from calibration curve (mol/L)= 2.25 x 10-5 Now I need to know: 1. moles FeNCS2+ at equilibrium (10mL) (mol) 2. moles Fe3+, reacted (mol) 3. moles Fe3+, equilibrium (mol) 4. [Fe3+] equilibrium, unreacted, 10 mL (mol/L) 5. moles SCN-, reacted (mol) 6. Moles SCN-, equilibrium (mol) 7. [SCN-] equilibrium (unreacted) 10 mL (mol/L) Feel free to just give me the formula to find these. Or to charge me 2 or 3 questions if I asked too much. Thank you!!!!!!