The pH of a solution made by mixing 50.0 mL of 0.13 molar B, a weak base, with 20.0 mL of 0.19 M HCl is 8.51. What is Kb for the weak base, B?
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- A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of solution. What is the pH of the solution after 0.368 mol of HX is added?A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
- A solution is prepared by mixing 80 mL of 0.2 M KH2PO4 and 120 mL of 0.2 M K2HPO4 . What is its pH?The pH value of the 5L aqueous solution prepared with 6.4 grams of a precious strong acid is 2. So what is the molar mass of the acid?A 0.450 M solution of a weak base has a pH of 9.55 What is the base hydrolysis constant, ?b, for the weak base?
- If a buffer solution is 0.180 M in a weak base (Kb=7.5×10−5) and 0.400 M in its conjugate acid, what is the pH?You combine 50.0 mL of 0.500 M NaOH with 75.0 mL of H2S04 with a Molarity of 0.19598. What is the resulting pH of the solution?If 10 mL of 0.1 M hypothetical acid, HA, is added with 10 mL of 0.1 M of the salt of its conjugate base, XA, what is the pH of the solution?
- A student added 1.78g of Ca(OH)2(9) to 0.250 L of 0.200 molL-1 HNO3(aq)- The mixture was carefully stirred until no further reaction occurred. Assuming that the total volume of the solution remains unchanged, calculate the pH of the resulting solution.At 250°C, the equilibrium constant for the dissociation of water is 10–11.16. At this temperature, what is the pH of a neutral solution?Calculate the pH of a solution that is 0.080 M pyridine (pKb = 5.25) and 0.285 M pyridinium chloride.