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(1) A sample of the hydrate CuSO4.5H2O has a mass of 12.5g.
(a) how many molecules of hydrogen are contained in this hydrate? If the hydrate is completely dehydrated.
Arrange the following aqueous solutions in order of deceasing freezing points: 0.10 m KNO3,0.10 m BSCl2,0.10 m ethylene glycol [C2H4(OH)2,antifreeze], and 0.10 m Na3PO4. Explain.
Determine pH of the solution....ICE table..Henderson HasselBach equations, Using a ICE table (initial change equilibrium) a)Calculate the pH of solution that is 0.175M in acidic acid(HC2H3O2) ans 0.110Min potassium Acetate(KC2H302)
What is the change in internal energy (in J) of a system that absorbs 6.03 kJ of heat from its surroundings and has 4.70 kcal of work done on it? 1 kcal = 4.184 kJ
explain the interaction effect between nitrogen and phosphorus and nitrogen and potassium. describe the dynamics amoung
What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted with pure water to a total volume of 0.15 L
In standardizing an unknown NaOH solution, 21.50 mL of NaOH solution are found to reach the endpoint in a titration with 0.792 g of KHP. (MW= 204.32.0 g/mol) What is the molarity of the NaOH solution
calculate the minimum number of grams of C3H8(g) that must be combusted to provide the energy necessary to convert 2.93 kg of H2O from its solid form at -13.0°C to its liquid form at 75.0°C.
Explain the pH change when the strong acid was added to the prepared buffer solution in relation to the pH of the buffer solution . Also indicate the change in the ph when the acid was mixed with the deionized water in relation to the deionized wa..
a beaker with 115 of an acetic acid buffer with a ph of 5.00 is sitting on a benchtop. the total molarity of acid and
write the balanced chemical equation for each of the following equilibrium constant expressions: a)Kc=[CO2][H2]/[CO][H2O. b)Kc=[H2][F2]/[HF]^2. c)Kc=[O2][HCl]^4/[Cl2]^2[H2O]^2. d)Kc=[CS2][H2]^4/[Ch4][H2S]^2.
Calculate the pH of a solution made by adding 51 g of sodium acetate, NaCH3COO, to 18 g of acetic acid, CH3COOH, and dissolving in water to make 700. mL of solution. Hint given in feedback.
Pure water is at equilibrium with excess CaCO3 (s) and MgCO3 (s). If the water has a pH of 8.61 and is open to the atmosphere (CO2 = 390 ppmv), calculate [Ca2+] and [Mg2+]. (for MgCO3 (s), pKs = 7.45)
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