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The following chemical equilibria are studied in this experiment. To become familiar with their behavior, indicate the direction, left or right, of the equilibrium shift when the accompanying stress is applied to the system. a. NH3(aq) is added to Ag+(aq) + Cl-(aq) -><-(double arrow) AgCl (s) b. HNO3(aq) is added to Ag2CO3(s) -><- Ag+(aq) + CO3 2-(aq) c. KI(aq) is added to Ag+(aq) + 2NH3(aq) -><- [Ag(NH3)2]+(aq) d. Na2S(aq) is added to AGI(s) -><- Ag+(aq) + I-(aq) e. KOH(aq) is added to CH3COOH(aq) + H2O(l) -><- H3O+(aq) + CH3CO2-(aq) f. HCl(aq) is added to 4 Cl-(aq) + Co(H2O)6 2+(aq)-><- CoCL4 2-(aq) + 6 H2O(l)
What color is the acetic acid plus methyl orange after addition of sodium acetate solution and what does this tell you about
Iodine-131 is used in medicine to assess thyroid gland function. How many protons and neutrons are present in an iodine-131 atom?
Three manufacturers are producing carbonated bottled water. One company introduces carbonate by bubbling carbon dioxide into water until CT=10-3 M (equivalent to adding "H2CO3*" until CT = 1 x 10-3 M), a second adds sodium bicarbonate (NaHCO3) unt..
Important information about balanced chemical equation, 1. If 1 mole of Al4C3 has a mass of 144g and carbon has a mass of 12g, what is the atomic mass of aluminum?
Calculate the pH of the solution that results from adding 28.0ml of 0.100M NaOH to 50.00 mL of a 0.0500 M solution of hydrochloric acid
Calculate the heat absorbed by 15.0 g of water to raise its temperature from 20.0oC to 50.0oC at constant pressure. The specific heat of water is 4.18 J/g.oC
The two occuring isotopes of gallium-69 and gallium-71,which are found in the ratio of 3:2. Determine the atomic mass of gallium.
A solution of glycerol in 701 g of water has a boiling point of 103.8 C at a pressure of 760 mm Hg. What is the mass of the glycerol in the solution?
How many moles of sodium chloride are present in the original solution. How many moles of ammonia are present originally
How do you calculate the pH when 0.2 moles of NaOH have been added to 1 mole of acetic acid during a titration. The pKa of acetic acid is 4.76.
Solve an equilibrium problem (using an ICE table) to calculate the pH of a solution that is 0.185 M in HC2H3O2 and 0.120 M in KC2H3O2
You take 1 ml of your sample and dialyze it in 1000 ml of buffer. At the end of dialysis what is the concentration of (NH4)2SO4 in your sample. How could you further lower the (NH4)SO4 concentration
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