What is the pH of a salt solution prepared by dissolving 0.00544 moles of LiX in enough water to form 16.00 mL of solution? The Ka of HX is 3.9 x10-6.
What is the pH of a salt solution prepared by dissolving 0.00544 moles of LiX in...
What is the pH of a salt solution prepared by dissolving 0.01368 moles of BaX2 in enough water to form 38.00 mL of solution? The Ka of HX is 8.4 10-7.
6. What is the pH of a solution prepared by dissolving 1.00 g of (CH3)2NH in enough water to form 500. mL of solution? What is the pH of this solution? 7. What is the molarity of hydronium ion and pH of 0.035 M ammonia solution? 8. Arrange following equimolar solutions in the order of increasing pH: NaCl, HF, NH3, and KOH. Explain your reasoning.
Calculate the pH of a solution prepared by dissolving 0.876 moles of carbonic acid (H2CO3) and 0.543 moles of sodium hydrogen carbonate (NaHCO3) in water sufficient to yield 1.00 L of solution. The Ka of carbonic acid is 4.5x10^-7. Explain answer please
What is the molarity (moles per Liter) of an aqueous solution that is prepared by dissolving 41.5 g of potassium iodide (KI; Molar Mass = 166.0 g/mole) in enough water to make 2,500.0 mL of solution? (5 points]
A solution was prepared by dissolving 0.200 moles of sodium hypoch lorite (NaClO) in water to a final volume of 1.00 Liter. Ka 2.96x10 for hypochlorous acid (HCIO). Show equations and work steps for these calculations. 1) Calculate Kb of sodium hypochlorite. 2) Calculate the pH of the NaClO solution. 3) Calculate the pH if 10.0 mL of 1.00 M HCl is added to 100.0 mL of the original NACIO solution. 4) Calculate the pH if 20.0 mL of 1.00...
A solution is prepared by dissolving 0.23 moles of chloroacetic acid and 0.27 moles of sodium chloroacetate in water sufficient to yield 1.00L of solution. The addition of 0.05 mole of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the.........present in the buffer solution. The Ka of chloroacetic acid is 1.36*10^-3.
What is the pH of a solution that is prepared by dissolving 7.20 grams of salicylic acid (formula weight = 138.12 grams/mol) and 7.12 grams of sodium salicylate (formula weight = 160.10 grams/mole) in water and diluting to 700.00 mL? The Ka for salicylic acid is 0.00105.
What is the pH of a solution that is prepared by dissolving 9.90 grams of pyruvic acid (formula weight = 88.06 grams/mol) and 9.25 grams of sodium pyruvate (formula weight = 90.04 grams/mole) in water and diluting to 800.00 mL? The Ka for pyruvic acid is 0.00324.
Determine Ka of the weak acid HX knowing that 0.10M
solution of LiX has pH of 8.90
Post-Laboratory Questions and Exercises DUE AFTER COMPLETING LAB. ANSWER IN SPACE PROVIDED. 1. Determine the K, of the weak acid HX knowing that a 0.10 M solution of LiX has pH of 8.90.
A scientist prepared a 0.037 M NH4Cl salt solution by dissolving the solid salt in water. Calculate the pH at 25°C for the solution, given that the Kb of ammonia, NH3, is 1.8 ✕ 10−5.