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- Calculate the concentrations of all species present (other then water) in an aqueous solution of 0.25 M H2SO3 Constants: Ka1,H2SO3= 1.5x10^-2 Ka2,H2SO3= 6.3x10^-8 Kw= 1.0x10^-14The pH of dissolving 1.48 g of propanoic acid (CH3CH₂COOH, Ka 1.3X105) in 200 mL H₂O is 4.82 3.71 2.94 1.22 5.25Calculate the concentration of all solution species in a 0.0500M solution of CaF2. KaHF=7.0x10-4.
- Kw for water at 100 degrees celsius is 49 x 10^-14. Calculate the concentration of hydroxide ions in pure water at 100 degrees celsius. a. 7.0 x 10-7 b. 0.0000001 c. 0.00000008 d. 2.2 x 10-7Bacteria in the human mouth release enzymes to break up sucrose, and thenpolymerize glucose to form a bacterial plaque. When this glucose is digested, it formslactic acid, which causes tooth decay. Tooth enamel is made of calcium phosphate.Lactic acid has a Ka 1.38x10 -4 and ionizes into lactate and H3O+ ions. Assuming aninitial lactic acid concentration of 0.10 mol/L on your tooth, determine the pH(assume a 1:1:1 mole ratio) and the percent ionization. Should people be concernedwith plaque buildup? Justify your answer.What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M? A 34.1 % (NH4 )2SO4 (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) NEED HELP ASAP NO WORK NEEDED
- The average density of sea water is 1.02 g/mL. If sea water contains an average of 260 ppm of sulfate ions (96.06 g/mol), calculate the molar concentration of sulfate ions for sea waterThe average density of sea water is 1.02 g/mL. If sea water contains an average of 260 ppm of sulfate ions (96.06 g/mol), calculate the molar concentration of sulfate ions for sea waterFor a solution that is 0.20 M in oxalic acid (H2C2O4), write the reactions for the ionization of this diprotic acid. The acid ionization constants are Ka1= 6.5 x 10^-2 and Ka2= 6.1 x 10^-5. Calculate the pH, [HC2O4-] and [C2O42-].Suppose each circle below represents a container of an aqueous solution of three differentacids, HA (Ka = 1 × 10−3), HB (Ka = 1 × 105), and HC (Ka = 1 × 10−8). Draw a representativeparticulate level diagram of all the predominant species, and their relative quantities, atequilibrium if the initial concentrations of all three solutions were the same. Omit watermolecules for clarity.
- With the use of ICE, calculate the % ionization of the solute in 0.1M HNO2 solution. Ka = 4.5x10-41. Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine is 1.8 x 10-9. The answer must be given with the correct number of significant figures. 2. How many grams of NaF must be added to 60.0 mL of 0.500 M HF(aq) to adjust the pH to 3.40? Assume no volume change. The pKa of HF is 3.14.Write the equations that represent the first and third ionization steps for phosphoric acid (H3PO4) in water. (Use H3O+ instead of H+.) first ionization step: + H2O(l) + third ionization step: + H2O(l) + --- The value of Ka for acetic acid is 1.80×10-5.What is the value of Kb, for its conjugate base, CH3COO-? --- The value of Ka for nitrous acid is 4.50×10-4.What is the value of Kb, for its conjugate base, NO2-?