1. 12/14 points Last Response | Show Details All Responses Notes a. During your lab, you prepared a reaction table for 10.0 mL of 0.1 M NH4Cl with 5.0 mL of 0.1 M NaOH.Please choose all of the following that describe the solution that was produced. [_] [x] A solution containing a weak acid and a weak base. [_] [_] A solution containing a weak base and a strong acid. [_] [_] A solution containing only a strong acid. [_] [_] A solution containing a strong acid and a strong base. [x] [_] A solution containing only a weak acid. [_] [_] A solution containing only a strong base. [_] [_] A solution containing a weak acid and strong base. [_] [x] A solution containing a conjugate acid/base pair. [_] [_] A solution containing only a weak base. [_] [x] A buffer.b. Complete the reaction table for the mixture of 10.0 mL of 0.10 M NH4Cl with 10.0 mL of 0.10 M NaOH below. All entries should be in millimoles. Report all values to one decimal place.NH41+(aq) + OH1-(aq) NH3(aq) + H2Oinitial1.0 [1.0] 1.0 [1.0] 0 [0]-1.0 [-1.0] -1.0 [-1.0] 1.0 [1.0]final0 [0] 0 [0] 1.0 [1.0]c. Calculate the equilibrium concentration of NH3 to two significant figures.[NH3] = 0.05 [0.05] Md. Please choose all of the following that describe the solution that was produced.[_] [_] A solution containing a conjugate acid/base pair. [_] [_] A solution containing a weak base and a strong base. [_] [_] A solution containing only a strong acid. [_] [_] A solution containing a strong acid and a strong base. [_] [_] A solution containing a weak acid and a weak base. [_] [_] A solution containing a weak base and a strong acid. [x] [x] A solution containing only a weak base. [_] [_] A solution containing a weak acid and strong base. [_] [_] A solution containing only a strong base. [_] [_] A buffer. [_] [_] A solution containing only a weak acid.e. Complete the reaction table for the mixture of 10.0 mL of 0.10 M NH4Cl with 15.0 mL of 0.10 M NaOH below.All entries should be in millimoles. Report all values to one decimal place.NH41+(aq) + OH1-(aq) NH3(aq) + H2Oinitial1.0 [1.0] 1.5 [1.5] 0 [0]-1.0 [-1.0] -1.0 [-1.0] 1.0 [1.0]final0 [0] 0.5 [0.5] 1.0 [1.0]f. Calculate the equilibrium concentration of NH3 to two significant figures. [NH3] = 0.040 [0.040] Mg. Please choose all of the following that describe the solution that was produced. [x] [x] A solution containing a weak base and a strong base. [_] [_] A solution containing a conjugate acid/base pair. [_] [_] A solution containing a weak acid and strong base. [_] [_] A solution containing a weak base and a strong acid. [_] [_] A solution containing only a strong acid. [_] [_] A solution containing only a strong base. [_] [_] A solution containing a weak acid and a weak base. [_] [_] A solution containing a strong acid and a strong base. [_] [_] A solution containing only a weak acid. [_] [_] A solution containing only a weak base. [_] [_] A buffer.2. 5.5/5.5 points Last Response | Show Details All Responses Notes Please calculate the pH of each of the following aqueous solutions. Report all pH's to two decimal places. a. 10.0 mL of 0.1 M NH4Cl plus 10.0 mL of 0.1 M NaOH pH = 10.97 [10.98] b. 10.0 mL of 0.1 M NH4Cl plus 15.0 mL of 0.1 M NaOH pH = 12.30 [12.30] 3. 5.5/5.5 points Last Response | Show Details All Responses Notes Please calculate the pH of each of the following aqueous solutions. Report all pH's to two decimal places. a. 10.0 mL of 0.1 M NaC2H3O2 plus 10.0 mL of 0.1 M NaOH pH = 12.70 [12.70] b. 10.0 mL of 0.1 M NaC2H3O2 plus 15.0 mL of 0.1 M NaOH pH = 12.78