The Solubility Product Constant for barium phosphate is 1.3x10-29. If barium phosphate is dissolved in water you can say that the equilibrium concentrations of barium and phosphate ions are: A. High B. Moderate C. Low The solubility of barium phosphate in water is: A. High B. Moderate C. Low

Consider the following chemical reaction.                           H2(g)  +  I2(g) ---> 2 HI(g)               At equilibrium, the concentration of H2, I2 and HI were found to be .20M, .044M, and .74M respectively.  What is the value of Kc for this reaction?                           Group of answer choices 23 112 62 .0089

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How will the equilibrium shift if the following changes are made? State if the reaction will shiftto the left or right and explain why it will shift in that direction. PCl5 (?)+heat ⇌ PCl3 (?)+ Cl2 (?) a.Temperature is increased b. Pressure is increased c. Cl2 is added d. PCl3 is removed as it is formed

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Heating solid sodium bicarbonate in a closed vessel established this equilibrium: 2NaHCO3(s) → Na₂CO3(s) + H₂O(g) + CO₂ (g) What would happen to the equilibrium position in the following situations (the temperature remains constant)? Part 1 of 3 Some of the solid NaHCO3 was removed from the system. O shift equilibrium to the right O have no effect O shift equilibrium to the left X

value for silver sulfate. The solubility of Ag,SO4 is measured and found to be 5.15 g/L. Use this information to calculate a Ksp Ksp

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