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Interpretation:
The
Concept Introduction:
It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.
If the value of
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Chapter 10 Solutions
Pearson eText Fundamentals of General, Organic, and Biological Chemistry -- Instant Access (Pearson+)
- Consider the titration of 30.0 mL of 0.0700 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HI. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH = (b) 5.3 mLpH = (c) 10.5 mLpH = (d) 15.8 mLpH = (e) 21.0 mLpH = (f) 27.3 mLpH =arrow_forwardCalculate the normality of a solution that contains 4.5 g of (COOH)2 in 3000 mL of solution? (Assume the (COOH)2 is to be completely neutralized in an acid-base * reaction.) 0.033 N O 0.33 N O 0.166 N O 0.0166 N 0.45 N O 0.045 N 000.0 OOarrow_forwardGiven the titration curve of the hypothetical polyprotic acid X at 0.100 M concentration (pKa1=4.0, pKa2=8.0, pKa3=12.0) titrated with 0.600 M NaOH, identify the pH at point C, H, E, and M.arrow_forward
- Quinine ( C20 H24 N2 O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pK, = 5.1 and pK, = 9.7 ( pKp = – log Kp). Only 1 g quinine will dissolve in 1920.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction | Q+ H2O= QH+ + OH- described by pK, where Q = quinine. pH =arrow_forwardDescribe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NAOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pK, of glycine is 9.6.arrow_forwardWhat is the m/v % concentration of a solution of LiCl with a density of 2.07 g/mL in 40.0 mL of deionized water with a density of 1 g/mL?arrow_forward
- Assuming the molar extinction coefficient for para-nitrophenyl phosphate (PNP) is 55,290 mol "dm cm, calculate the concentration of the molecule that produced an absorbance of 0.770 OD units in a 1.5 cm cuvette. Show all working -1 3 -1arrow_forwardWhat is the pH of a 0.25 M solution of acetic acid, Ka = 1.8 x 105. What percentage of the acid is dissociated?arrow_forwardDescribe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NaOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pKa of glycine is 9.6arrow_forward
- The-carotene molecule has λmax 450 nm and ɛ = 15.000 m2 / mol. Calculate the expected absorbance value for a solution in which 0.1 mg is dissolved in 10 mL of water. ( β-carotene, C40H56, 536 g/mol path length 1 cm)arrow_forwardTitration of a 12.0 mL solution of HCl requires 22.4 mL of 0.12 M NaOH. What is the molarity of the HCl solution?arrow_forwardThe main constituents in vinegar are water and ethanoic acid (CH3COOH). In order to determine the concentration of acid in homemade vinegar, a student titrated 25 cm3 of 001 M NaOH against the vinegar. The equation for the reaction is: CH3COOH(aq) + NaOH(aq) ® CH3COONa(aq) + H2O(l) The following titration results were obtained: Burette readings (cm3) Rough 1 2 Final burette reading 20.10 38.90 31.40 Initial burette reading 0.10 20.00 12.50 Volume of vinegar used 20.00 18.90 18.90 (a) What volume of vinegar should be used in the calculation? (b) What is the mole ratio of NaOH:CH3COOH? (c) Calculate the number of moles of alkali in 25 cm3 of NaOH solution used. (d) How many moles of acid were used in the titration? (e) Calculate the…arrow_forward
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