Calculate the ionic strength (j) for a) the solution of AlCl3 (0.01 N) + Ca(NO3)2 (0.002 M) (A=0.51) b) the solution of CH3COOH 0.01 M , Ka = 10-5 M (A=0.51)
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Calculate the ionic strength (j) for
a) the solution of AlCl3 (0.01 N) + Ca(NO3)2 (0.002 M) (A=0.51)
b) the solution of CH3COOH 0.01 M , Ka = 10-5 M (A=0.51)
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- Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH;NH2(aq) + HCIO3(aq) > 4- 3. 2+ 3+ 4+ 1 2 6 7 8 O2 4 5. ) (s) (1) (g) (aq) H N H30* CI H20 OH 4- +Balance the equation and choose the coefficient of the (?) NazCO3 + HCl → NaCl + H20 + CO2 -> (x)NA2CO3 + (x)HCl → (? )NaCl + (x)H20 + (x)C02Balance the equation and choose the coefficient of the (?) Na2CO3 + HCl → NaCl + H20 + CO2 -> (x)NA2CO3 + (?)HCl → (x)NaCl + (x)H20 + (x)CO2
- Does a precipitate form when a solution of calcium chloride and a solution of mercury(1) nitrate are mixed together? Choose one: O Yes, a precipitate is formed. O No, a precipitate is not formed.Dilution is necessary for commercially available acids such as HNO3, H2SO4 etc so that the strength is reduced to be used by students in a chemistry laboratory. Select one: O True O False0.6465 grams of bleach, Ca(OCl)2, is dissolved in acid and treated with excess KI. Calculate the weight percent of Ca(OCl)2 in the bleaching powder when the released iodine is titrated with 36.92 mL of 0.06608 M Na2S2O3 (MaCa(OCl)2: 143 g/mol). A. 6.74B. 13.48C. 20.22D. 26.96
- A 3.026 grams of Cu (II) salt is dissolved in water and then diluted to 250 mL in a volumetric flask. Iodine is liberated when one gram of KI solution is added to 50.0 mL of aliquot sample. A 23.33 mL of 0.04668 M Na,S,O, solution is required to titrate the iodine liberated. Calculate the weight percent of the Cu in the salt. (A) 11.43%, just before end point (B) 12.43%, just before end point (C) 11.43%, after equivalence point (D) 12.43%, after equivalence point(a) (1) CI AICI (2) HNO₂, H₂SO (3) O (4) Me,S (5) NaBH; H₂O+ एल Draw Your Solution(3) 11. In a titration it is found that 97.7 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of a solution of HCl(aq). Calculate the concentration of the HCl solution. Show your work. [Hint: Write a balanced equation for the reaction first.]
- 5.) Calculate the volume, in liters, of NaOH required to titrate the KHP in flask #2. (A7) – (A6) Volume of NaOH = 1000 mL/L 16.36 O.80 (A14) 1000 mL/L ||5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)Write the expression Kc for the following reactions. (a) Fe2+(aq) + Ce4+(aq) ⇋ Fe3+(aq) + Ce3+(aq) (b) CaCO3(s) ⇋ CaO(s) + CO3(g)