A students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH solution. What is the resulting pH?

A student dissolves 0.0100 mol of an unknown weak base in 100.0 mL of water and titrates the solution with 0.100 MHNO3. After adding 40.0 mL of HNO3, the pH of the resulting solution is 8.00. Calculate the pKb for the weak base.(a) 7.82 (b) 6.18 (c) 8.18 (d) 7.60

What is the pH of the solution after 50.00 mL of 0.100 M  NaOH  is added to 50.00 mL of 0.100 M acetic acid?

You are asked to find the pH of each solution described below. A 0.50 M solution of HBrO3 A 0.030 M solution of Ca(OH)2 A 0.50 M solution of NH4Br A solution that is 0.20 M in NH3 and 0.35 M in NH4NO3 after the addition of a small amount of NaOH A solution that is 0.40 M in HCOOH and 0.30 M in NaHCOO A 0.25 M solution of CH3NH2 Options： A.weak acid B.strong acid C.weak base D.strong base E.acid salt F.basic salt G.buff by it self H.buff after add strong base I.buff after add strong acid