A 46.9 mL solution of 0.419 mol L−1NH3 is titrated using 0.578 mol L−1HCl. What volume of HCl (in mL ) is needed to rea
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Consider a 1.0 L buffer containing 0.086 mol L−1HF and 0.097 mol L−1 F. What is the pH of the solution after adding 6.6×10−3 mol of HCl ? Express your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15 . They are also posted on eClass. Answer:
A 16.8 mL solution of 0.100 mol L−1NaOH is titrated using 0.150 mol L−1HCl. What is the pH of the solution after 16.8 mL of the HCl solution is added? Express your answer to 2 decimal places. Answer:
A 10.5 mL solution of 0.100 mol L−1HF is titrated using 0.150 mol L−1NaOH. What is the pH of the solution after 4.66 mL of the NaOH solution is added? Express your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15 . They are also posted on eClass. Answer:
What is the molar solubility (in mol L L−1 ) of a salt in pure water with general molecular formula MX2 (where M is a cation and X is an anion) that has Ksp=7.63×10−11 ? Remember, if you want to express an answer in scientific notation, use the letter "E". For example " 4.32×104− should be entered as "4.32E4". Answer: