A 20.00 mL sample of 0.150 M NH3 is being titrated with 0.200 M HCl. What is the pH after 10.00 mL of HCl has been added? Kb of NH3 = 1.8 × 10−5

What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 4.00? (Ka for HF is 6.8 × 10⁻⁴)

Calculate the volume of 0.150 mol /L Ba(OH)2 necessary to neutralise 452 mL of 0.175 mol/L HCl.(First balance the neutralisation equation carefully.)

The pH of solution formed by mixing 40 mL of 0.10 M HCl and 10 mL of 0.45 M of NaOH is

Calculate pH of a 0.000375 M HCl solutionGroup of answer choices- 3.4333.753.43

Correct order of boiling points of the given liquids is:A. H2O > HF > HCl > NH3B. HF > H2O > HCl > NH3C. HF > H2O > NH3 > HClD. H2O > HF > NH3 > HCl