. Calculate the ionic strength of a solution containing 0.10 M NaCl and 0.20 M CaCl₂. Assume complete dissociation of both salts. a. 0.70 b. 0.30 c. 1.0 d. 0.50 gnibbs yd noitulos auosups moil moi griwollel ad attigist or ask o CSM daxil otaligioon lliw noi doidi onimplab o)
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- Which of the following statements is advantageous? A). The main differences between potentiometric and conductometric titrations are that potentiometric titrations exemplify the analyte sample-by-sample while conductometric titrations show the potential of the analyte B). A conductivity is analyl from the people of the charge. C.) Conductivity increases rapidly as close as equivalence, as a strong acid and a strong base will decrease D). The conductor remains constant according to the viscosity of the pixel, the decomposer and its size, which consists of design modelling.From the given information in the table calculate for both titration1 and 2: 1)moles of thiosulphate titrated (mols) 2) moles of hypochlorite (mols) 3) mass of sodium hypochlorite (g) 4) wt% of sodium hypochloriteWhat species are present in a solution giving off a pure blue endpoint in a hard water sample containing an EBT indicator (In) with an EDTA titrant? a. HIn²⁻, CaY²⁻, MgY²⁻ b. HIn²⁻, MgIn⁻, CaY²⁻, MgY²⁻, CaIn⁻ c. HIn²⁻, MgIn⁻ d. HIn²⁻, MgIn⁻, CaY²⁻
- calculations for acetate buffer solutions 1. moles of sodium acetate in in 250.0 mL acetate buffer (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solvingequal volumes of 0.15M sulfurous acid and 0.3M potassium hydroxide are moxed. write net ionic and identify spe ies with highest concentration at equlibrium. Please explain justification
- Calculate the solubility of CaF2 (aq) in a solution, that is 0.015 molar in MgSO4 (aq). Compare your result to the one you obtain by using concentration instead of activities. Take the solubility product as 3.9 × 10 ^-11Calculate the alkaline strength of pearl ash (impure potassium carbonate) in terms of percent K2O from the following data: Sample = 0.3500 g; HCl used = 48.03 mL; NaOH used for back titration = 2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4.H2O. (Note: Use the least significant digits in your answer.)For µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µg
- A 50-mL solution of 0.5005 N standard NaOH was added to a 0.9250-g sample of Aspirin and was boiled for 10 minutes. After cooling a full pipet of phenolphthalein was added to the solution before it was titrated with 24.7 mL of 0.5015 N standard HCl solution until the disappearance of the pink color. The same procedure was carried using a blank which consumed 4.6 mL of the same standard acid. Calculate for the %Aspirin in the sample. Atom weights: C =12, H =1, O =16.Calculate the alkaline strength of pearl ash (impure potassium carbonate) in terms of percent K2O from the following data: Sample = 0.3500 g; HCl used = 48.03 mL; NaOH used for back titration = 2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4.H2O.A 250.0mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091M NAOH , requiring 29.5ml to reach end point. Determine equivalent weight