7-43. Supply the missing data in the table below. Molar Analytical Concentration, cT Acid (cr = cHa + ca-) pH (HA] [A¯] Lactic 0.120 0.640 lodic 0.200 0.765 Butanoic 5.00 0.0644
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- 7-43. Supply the missing data in the table below. Molar Analytical Concentration, c- (ct = Cha + cx-) pH (A"] Acid (HA] Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 0.145 0.221 Hydrogen cyanide Sulfamic 0.250 1.205. a) The Kw value that we normally use is for room temperature (25°C). Calculate the equilibrium H+ concentration and pH of pure, neutral water at 0.0°C (Kw= 1.14 x 10-15at 0.0°C) b) Methylamine (CH3NH2) is a derivative of the weak base ammonia. Write the equation for the ionization of methylamine in water, and use the I.C.E. method to find the pH of a 3.75 M CH3NH2 solution.(Kb= 4.37 x 10-4at 25°C)How to write the methodology? I have a practical of the MEASUREMENT USING PH METER, I don't know how to write the methodology. Here is the introduction: A pH meter is an electronic device mainly used for qualitative measurement, for thedetermination of acid and the basic value of a solution. Generally, it measures thehydrogen ion concentration/activity [H+] in a solution. It is denoted as:pH = - log10 [H+]In a pure water solution, the concentration of [H+] and [OH-] ions, respectively, rangefrom 1.0 x 10-1 M to 1.0 x 10-14 M. When [H+] is equal to [OH-] as when pure waterdissociates, the hydrogen ion concentration of pure water is equal to 1.0 x 10-7 M orpH = 7.00, defined as a neutral solution at 25°C, to be of temperaturedependent/endothermic dissociation.[H+] = [OH-] = 1.0 x 10-7 MWhen an ionic or polar substance is dissolved in water, it may change the relativenumbers of H+ and OH-. The higher the pH number, the lower the hydrogen ion concentration, and vice versa. Solution with an…
- Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O (m = NH4*(aq) + OH-(aq) At 25°C, Kb, is 1.8 × 10-5 (7) Calculate the pH of a mixture of 0.192 mol NH3 and 0.116 mol NH4C1 diluted to 400.0 mL with distilled water.Ex. 13-5. A 50.00-mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocresol green indicator. Calculate the molarity of the HCl. Ва(ОН)2 + 2HCІ- ВаCl, + 2H-0Full 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.
- 7:30 1 y short X Powe X RI Anno x ! Ceng x PI TURUE A TINA A y weba x Piese y chem 101 Chem X i app.101edu.co Time's Up! Construct the expression for Ka for the weak acid, HCN. HCN(aq) + H.O(1) = H.O (aq) + CN (aq) Based on the definition of Ka, drag the tiles to construct the expression for the given acid. Ka = 5 RESET [H:O] [H.O'] [OH] [HCN] [H:CN') [CN] 2[H:O] 2(H.O) 2[OH] 2(HCN] 2[H.CN'] 2(CN] [H:OP [H.O'P [OHP [HCNJ" [H:CNP [CNPIn the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
- A solution of acetic acid CH3COOH, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.68, what was the initial concentration of the acid? Ka=1.7x10-5 Ethanolamine, HOC2H4NH2, is a viscous liquid with an ammonia-like odour used to remove hydrogen sulphide from natural gas. A 0.15 mol dm-3 aqueous solution of ethanolamine has a pH of 11.34. What is kb for ethanolamine? What is the concentration of hydroxide ion in a 0.060 mol dm-3 aqueous solution of methylamine, CH3NH2? What is the pH? Kb=4.4x10-412) Calculate the [H*], pH, and pOH for a 100.00mL of 0.00250M HCI at 25°C. [H*] = pH pOH = M %3DThe pH for 0.0850 M solution of CoHsCH2COOH is 2.68. Determine the value of Ka for CoHsCH2COOH. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C&H:CH2COOH(a_ H2O(1) H;O*(aq) CoHsCH2CO0 (aq) q) Initial (M) Change (M) Equilibrium (M) RESET 0.0850 2.68 -2.68 2.1 x 10-3 -2.1 x 10 3 0.0829 -0.0829 0.428 -0.428 +x 2.68 + x 2.68 - x 2.1 x 10-3 + x 2.1 x 10-3-x 0.428 + x 0.428 x