a. Calculate the degree of ionization of 0.25 M HCHO2 (formic acid) solution. K. (formic acid) = 1.7 x 10-4 Degree of ionization =| b. Calculate the degree of ionization of 0.25 M HCHO, (formic acid) solution that is also 0.30 M HCI. %3D K. (formic acid) = 1.7 × 10-4 Degree of ionization =
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- Full 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.a) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.Using the known value for the Ka for acetic acid (1.76x10^-5),calculate the expected ph of an acetic acid solution with a concentration equal to that found in this experiment(I.e the concentration you determined) which was .8604
- Calculate Kb for a 0.1 M solution of acetate ion, given that Ka for acetic acid is 1.8 x 10−5. Group of answer choices 5.56 x 10−10 6.4 x 10−6 7.4 x 10−8 8.4 x 10−9 1.8 x 105 4.24 x 10−3 1.34 x 10−3Calculate the molar solubility of zinc carbonate in ZnCO3(s) Zn2+(aq) + CO32-(aq) Kps=3.10-8 Water: solubility = [ ] mol.L-1 • Zn (NO3) 2 solution 0.0500 mol.L-1: solubility = [ ] mol.L-1 • K2CO3 solution 0.0500 mol.L-1; solubility = [ ] mol.L-1This is the answer I got for this problem, but It's saying I have the change in concentration wrong. I don't understand what the help prompt is saying here. I also have Ka = 2x/(0.015-x) = 0.0003 Is that correct? It didn't fit on the snip I took, sorry.
- Using the Henderson-Hasselbalch equation (see your class notes), calculate the pH of the solution containing 1.0M HC2H3O2 and 1.0M NaC2H3O2. The Ka of HC2H3O2 is 1.8x 10-5. Show your work in the space provided.Ka for ethanoic acid is 1.7*10^-5 moldm-3. Show by calculation that the initial pH in experiment B is 4.8.Explain why the pH of mixture C is the same as the pH of mixture A C) Mixture made by mixing equal volumes of 0.2 mol L–1 HCl and 0.2 mol L–1 NaCl Conductivity (mA) 340 PH 1 A 0.1 mol L–1 HCl 260 1
- The solubility of CaCO3 is pH dependent. (a) Calculate themolar solubility of CaCO3 (Ksp = 4.5 x 10-9) neglectingthe acid–base character of the carbonate ion. (b) Use the Kbexpression for the CO32 - ion to determine the equilibriumconstant for the reactionCaCO3(s) + H2O(l) ⇌ Ca2 + (aq) + HCO3-1 (aq) + OH-1 (a q)(c) If we assume that the only sources of Ca2 + , HCO3-,and OH- ions are from the dissolution of CaCO3, what is the molar solubility of CaCO3 using the equilibrium expressionfrom part (b)? (d) What is the molar solubility ofCaCO3 at the pH of the ocean (8.3)? (e) If the pH is bufferedat 7.5, what is the molar solubility of CaCO3?Which of these procedures would not make a pH =4.75buffer?(a) Mix 50.0 mL of 0.10 M acetic acid and 50.0 mL of 0.10 M sodium acetate.(b) Mix 50.0 mL of 0.20 M acetic acid and 50.0 mL of 0.10 M NaOH.(c) Start with 50.0 mL of 0.20 M acetic acid and add a solution of strong base until the pH equals 4.75.(d) Start with 50.0 mL of 0.20 M HCl and add a solution of strong base until the pH equals 4.75.(e) Start with 100.0 mL of 0.20 M sodium acetate and add 50.0 mL of 0.20 M HCl.A particular solution is 0.05M with respect to ethanoic acid and 0.2M with respect to sodium ethanoate (Ka for ethanoic acid = 2 x 10-5moldm-3). What is this type of solution called? Calculate the pH of the solution