Calculate the pH and concentrations of CH, NH, and CH, NH; in a 0.0363 M methylamine (CH, NH,) solution. The Kp of CH, NH, is 4.47 x 10 4. pH = %3D (CH, NH,] = M. !3D [CH, NH; ]
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![Calculate the pH and concentrations of CH, NH, and CH, NH; in a 0.0363 M methylamine (CH, NH,) solution. The Kp of
CH, NH, is 4.47 × 10 1.
pH
(CH, NH,
%3!
M
[CH, NH;]
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- The hydronium ion concentration of an aqueous solution of 0.591 M aniline (a weak base with the formula C,H5NH,) is ... [H;O*] = М.The hydronium ion concentration of an aqueous solution of 0.591 M aniline (a weak base with the formula CH5NH,) is ... [H3O*] = М.The hydronium ion concentration of an aqueous solution of 0.558 M isoquinoline (a weak base with the formula CoH-N) is ... M. = LO°H]
- (c) after adding 0.030_mol of HCI to 1.0 L of the buffer solution in part (a) 0.030mol [H;O*]addea Step 1. Use Stoichiometry to calculate new concentrations Concentration (M) CH;COO-(aq) + H;O*(aq) = 0.030M %3D 1.00L solution CH,COOH(aq) + H,O (1) Initial 0.40 0.030 0.40 Change Final Step 2 Set up a reaction table with the new concentrations. Concentration (M) CH,COOH(aq) + H2O(1) + CH;COO((aq) + H;O*(aq) Initial Change EquilibriumNH3 is a weak base. It ionizes in water to produce NH4+ and OH-. Its Kb = 1.8 10-5 and Kw = 1 10-14 at 25oC. Please complete following tasks for a solution of 0.0500 M NH3 (aq) at 25oC. (a) ionization % of NH3, (b) pH of this solution, (c) concentration of OH- ; and (d) concentration of NH4+What is the concentration (in molarity) of H*, HCO3, and CO32-, in a solution that is initially prepared as a mixture of 0.0100 M H2CO3 and 0.000010 M Na2CO3? (Carbonic acid is a weak diprotic acid where Ka1 is 4.20 x 10-5 and K,2 is 2.00 x 10-6) a) [H'] at equilibrium = ? %D b) [HCO3] at equilibrium - ? c) [CO,] at equilibrium ?
- 8. Our bodies are able to preserve a near constant pH due to the presence of hydrogen carbonate anion (HCO,). K values for the diprotic acid carbonic acid (H,CO;) are Kaj = 4.5 x 10?, K2 = 4.7 x 10-". a) Hydrogen carbonate anion is an amphoteric species. Define amphoteric. b) In the space below, write out chemical equations to describe the behavior of this species as both a Bronsted acid and a Bronsted base, and use the equilibrium constants given above to decipher whether a solution of HCO;¯ will be acidic, basic, or neutral. Support your answer with pertinent calculations.(CH) NHC). A solution is prepared that is initially 0.17 M in trimethylamine ((CH, N, a weak base, and 0.20 M in trimethylammonium chloride Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in OH. You can leave out the M symbol for molarity. [(CH.),N] [CH.),NH] [oH] initial change final Explanation Check Rights Reserved. Privacy Accessibility 2021 McGraw-Hill Education V 1 10:4 acer oloIn the laboratory, a general chemistry student measured the pH of a 0.509 M aqueous solution of phenol (a weak acid), CGH5OH to be 5.162. Use the information she obtained to determine the K, for this acid. K„(experiment) =
- (a) Write the net ionic equation for the reaction that occurswhen a solution of hydrochloric acid (HCl) is mixed with asolution of sodium formate (NaCHO2). (b) Calculate theequilibrium constant for this reaction. (c) Calculate theequilibrium concentrations of Na+, Cl-, H+, CHO2-, andHCHO2 when 50.0 mL of 0.15 M HCl is mixed with 50.0 mLof 0.15 M NaCHO2.You did not divide by any reactants for Q. Is that becuase the concentration of HNO2 is 1 M? ...and if so, why would it not be 0.5M?In solutions 1-4 you are adding successively larger volumes of 0.00200 M SCN- to the Fe3+ solution and diluting to 10.00 mL. Calculate the final diluted molarity of SCN- in solution #1. 3 sig figs (Calculate the same thing for the solutions 2-4 and enter the results in table 3 as [SCN-] pre-equilibrium.)