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- What is the pH of a solution that is a prepared by dissolving 4.90 g of (NH4)2SO4 ( K₁ (NH4+) = 5.70 × 10-¹0) in water, adding 150.0 mL of 0.1263 M NaOH, and diluting to 900.0 mL? pH = b0.124 M in piperidine and 0.054 M in its chloride salt ( Ka (C5H₁1NH+) = 7.50 × 10−¹² )? -12 pH = C prepared by dissolving 2.12 g of aniline (93.13 g/mol, Ką (anilinium ion) = 2.51 × 10−5) in 100. mL of 0.0330 M HCl and diluting to 500.0 mL? pH =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 1.20(4c-201) Copy the following equation, and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid. HNO3 + H2O → H30* + NO3¬ For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial 14px A v ... In X2 田由田図 EX: ABC Ť {;} > >
- Calculate the pH and percent hydrolysis of a 0.25 mol L-1 solution of CH3NH3CI Kb(CH3NH2) = 4.4 x 10-4 Enter just the pH5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9
- 2-22. A 6.42% (w/w) Fe(NO,); (241.81 g/mol) solution has a density of 1.059 g/mL. Calculate (a) the molar analytical concentration of Fe(NO3)3 in this solution. (b) the mass in grams of Fe(NO;)3 in each liter of this solution.What is the pH of a solution of 0.400 M CH;NH2 containing 0.140 M CH;NH31? (Kb of CH3NH2 is 4.4 × 10-4)Ammonia (NH3) is a weak base with a Kp = 1.8 x 10-5. A certain solution of ammonia has a %3D pH = 9.05. What was the molar concentration of ammonia in the starting solution? %3D NH3(aq) + (H20(1) NH,*(aq) + OH (aq) And pH = JUL CC
- A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH)(COOH)(CH2COOH)2, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.Glutamine (HQ) is a diprotic amino acid with Ka = 6.5 x 10 and K = 1.00 x 10. Determine the pH of cach of %3D the solutions. A 0.172 M głutamine hydrochloride (H, Q*CI") solution. pH = A 0.172 M glutamine (HQ) solution. pH = A 0.172 M sodium glutaminate (Na*Q) solution. pH =7-43. Supply the missing data in the table below. Molar Analytical Concentration, c- Acid (Ct = CHa + Ca-) pH (HA] [A^] Lactic 0.120 0.640 Iodic 0.200 0.765 Butanoic 5.00 0.0644 Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 Hydrogen cyanide Sulfamic 0.145 0.221 0.250 1.20