A solution contains 0.300 g HC2H3O2 in 50.0 mL of water. (Ka = 1.80*10-5)  -What is the pH of the HC2H3O2 solution?  -What volume of 0.250 M NaOH must be used to reach the equivalence point?

Calculate the pH of a buffer solution prepared by dissolving .37 moles of formic acid (HCO2H) and .23 moles of sodium formate (NaCO2H) in 1.00 L of solution. (Ka = 1.8 x 10-4 )     Group of answer choices 2.09 2.30 10.46 3.54

Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc). Ka for HAc is1.8x10 -5.  How much NaOH must be added to reach the equivalence point, and what is the pH at the equivalence point?

A solution contains 0.351 M HA (Ka = 1.13⋅10−51.13⋅10-5) and 0.744 M NaA.   What is the pH of this solution?   What is the pH of this solution after 0.186 mol of HCl are added to 1.00 L of this solution?   What is the pH of this solution after 0.372 mol of HCl are added to 1.00 L of this solution?

What is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10-5) when 100.0 mL of a 0.0.75 M HCl solution is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ?Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.

Calculate the pH of a buffer solution containing 0.584 mol HA weak acid and 0.703 mol A- in 130.1 mL  after 0.158 g of NaOH was added? [Ka= 1.56 ×10-5] Report your answer with three decimals. Enter numbers only; do not enter units.

Given: A certain weak acid,HA with a Ka value of 5.61 •10-6 is tutorage's with NaOH.  part A: a solution is made by titration 7.00mmol of HA and 3.00 mmol of the strong base. What is the resulting pH? Part B: more strong base is added until the equivalence point is reached. What is the pH of this addition at the equivalence point if the total volume is 34mL?

A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. The ka of ammonia is 5.68 X 10-10.  The pKa of ammonia is 9.25.  These questions are challenging so this is very similar to the one online but the answers will be a little different.    What is the initial pH of the solution?     A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. What is the pH when 15.0 mL of HCl is added?      Calculate the pH at the equivalence point.         Calculate the pHat one-half equivalence point.       A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. What is the pH when 38.0 mL of HCl has been added?

We have 500.0 mL of a buffer solution which is 0.651 M in NH3 and 0.354 M in NH4Cl. 500.0 mL of a 0.224 M HCl solution are added. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the final pH of this solution?

A titration of a solution of a diprotic acid H₂C₃H₂O₄ (malonic acid) with 0.955 M NaOH required 82 mL to reach the second equivalence point. How many grams of malonic acid are present in the sample? (malonic acid MW = 104.06 g/mol)