Calculate the ionic strength of a solution containing 0.2 M NaCl in a 0.2 M Na2CO3. Consider all the ions in this solution in calculating the ionic strength.
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Calculate the ionic strength of a solution containing 0.2 M NaCl in a 0.2 M Na2CO3. Consider all the ions in this solution in calculating the ionic strength.
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- A chemistry graduate student is given 125.mL of a 0.40M ammonia NH3 solution. Ammonia is a weak base with Kb = 1.8x10−5. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.03? You may assume that the volume of the solution doesn't change when then NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.Which of the following has the lowest ionic strength? Group of answer choices 0.30 M Na3PO4 0.30 M NaCl 0.30 M Al2(SO4)3 0.30 M Na2SO4Calculate the total number of ions in 500 mL of 0.200 M K,S solution. Calculate the total number of ions in 500 mL of 0.200 M K,N solution. Calculate the total number of ions in 500 mL of 0.200 M KNO, solution. Calculate the total number of ions in 500 mL of 0.200 M K+ solution. Calculate the total number of atoms in 500 mL of 0.200 M KNO, solution.
- Using the square-bracket notation, express the concentration of chloride ions in a solution that is 0.250 M in sodium chloride(NaCl) and 0.25 M in magnesium chloride (MgCl2).4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.
- Calculate the concentration (molarity) of Pb2+ ions in a solution made by adding 0.010 moles of Pb(NO3)2 to 1.0 L of a 2.0 M NaI solution. (Kf = 3.0 x 104 for PbI42−) - 4.9 x 10−2 -3.3 x 10−5 - 2.1 x 10−7 -1.7 x 10−7 -2.3 x 10−8A chemistry graduate student is given 250. mL of a 1.40M ammonia (NH3) solution. Ammonia is a weak base with K-1.8x10 should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.17? What mass of NH, Br You may assume that the volume of the solution doesn't change when the NH4Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?Solubility of gases in water increases with increasing mass. Explain? What is the relationship between the value of pKa and the strength of a weak acid?
- Determine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.A standardized iodine solution is used to titrate hydrazine sulfate in a sodium bicarbonate- buffered solution. The reactions that occur are I2 + 2e- = 2I N2H4 .H2SO4 → N2 + SO4 2- + 6H+ + 4e- What is the molarity of a solution of hydrazine sulfate when 27.29 mL of 0.100 N iodine is required to titrate 25.00 mL of the hydrazine sulfate to the equivalence point?A solution of ammonium sulfate was prepared by dissolving 55.44g of (NH4)2SO4 in enough water to prepare a 2.00L solution. What is the concentration of ammonium ions in this solution?