Each row of the table below describes an aque Complete the table. That is, fill in any missing digits. [1,0] solution pH - 12 mol/L 9.1 X 10 ||mol/L 7.13 6.7 × 10 mol/L
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O ACIDS AND BASES
Interconverting pH and hydronium ion
Each row of the table below describes an aque
Complete the table. That is, fill in any missing
digits.
[1,0]
solution
pH
- 12
mol/L
9.1 × 10
||mol/L
7.13
9.
mol/L
C
6.7 X 10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2502842a-dd4f-42fe-b3b0-e6b02798da5f%2F566abd20-9c01-4c63-89d0-92fd51ca0c72%2Ftbtndgq_processed.jpeg&w=3840&q=75)
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- Ka for ethanoic acid is 1.7*10^-5 moldm-3. Show by calculation that the initial pH in experiment B is 4.8.What hydrogen ion concentration (H+) (expressed in mol dm - 3 ), corresponds-to a pH of 2.60? Give your answer to two decimal places and in scientific notationWhat is the pKa of the conjugate acid of a base that has a Kb value equal to 2.1 × 10-7? Report your answer to the hundredths place. Assume the temperature is 25ºC.
- Kb for methylamine at 25°C is 4.4 x 10-4 what is its pH if 0.10M solution is used.Calculate the concentration (M) of the anion Z2- for a 0.100 M solution of H2Z given the acid ionization constants for the acids below. Report your answer to the tenths place using scientific notation and do not include units. (ie. 1.1e+9, 1.1e-9) H2Z(aq) Ka = 7.8 x 10-2 HZ-(aq) Ka = 7.0 x 10-9please help me answer a nad then b a. In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of ethylamine, C2H5NH2 to be 12.185. Use the information she obtained to determine the Kb for this base. Kb(experiment) =______ b. Now, Write the Ka expression for an aqueous solution of nitrous acid: (Note that either the numerator or denominator may contain more than one chemical species. Enter the complete numerator in the top box and the complete denominator in the bottom box. Remember to write the hydronium ion out as , and not as ) Ka =
- 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.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.Some H2PO4- and HPO42- are added to water such that the concentration of each is the same value, 5.25 mmol L-1 (pKa = 2.1, 6.8, 12.4). The water was initially at pH 6.55 and 25.0 °C. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)
- Write equilibrium showing the carbonate anion (CO32-) acting as a Brønsted base in aqueous solution. Identify the conjugate base-acid (or acid-base) pairs and write the appropriate base dissociation constant (Kb) expression. Look up Kb value and compare to Kb of carbonate as 2.1 x 10-4. Did your value fall in the same range?The pKa values of some hypothetical acids (HX, HY, HZ, HG) are shown below: HX pka=2.50, HY pKa=4.72, HZ pKa=1.87, HG pKa=5.67 Which of the following conjugate bases will be the weakest? a) X- b)Y- c)Z- d)G- e)they all have the same strength P.S could you please tell me which concept it is or a topic?Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its conjugate base is pink in solution. Define the term" WEAK ACID"