Be sure to answer all parts. If 2.10 g of CuSO4 is dissolved in 8.75 × 102 mL of 0.310 M NH3, calculate the concentrations of the following species at equilibrium.
Cu2+ × 10 M Enter your answer in scientific notation.
NH3 M
Cu(NH3)42+ M
Be sure to answer all parts. If 2.10 g of CuSO4 is dissolved in 8.75 ×...
Be sure to answer all parts. If 2.10 g of CuSO4 is dissolved in 9.05 x 102 mL of 0.380 M NH3, calculate the concentrations of the following species at equilibrium. Cu2+ 11.8 X L:14 V Enter your answer in scientific notation. NH3 Cu(NH3)42+
Be sure to answer all parts. If 2.25 g of CuSO4 is dissolved in 9.07 × 102 mL of 0.320 M NH3, calculate the concentrations of the following species at equilibrium. Cu2+ × 10 MEnter your answer in scientific notation. NH3 M Cu(NH3)42+ M
If 2.40 g of CuSO4 is dissolved in 8.79 × 102 mL of 0.300 M NH3, calculate the concentrations of the following species at equilibrium. Cu2+ × 10 MEnter your answer in scientific notation. NH3 M Cu(NH3)42+ M
If 2.30 g of CuSO4 is dissolved in 8.65 × 102 mL of 0.330 M NH3, calculate the concentrations of the following species at equilibrium. Cu2+ ___ × 10^__ M Enter your answer in scientific notation. NH3 ___ M Cu(NH3)4^2+ ___ M
The Ksp and Kf values are not given, I think: Kf = 5.0 X 1013 If 2.10 g of CusO, is dissolved in 9.21 x 10- mL of 0.350 M NH2, calculate the concentrations of the following species at equilibrium. Cu2+ x 10 M Enter your answer in scientific notation. NHz м Cu(NH3)42+ м
Please show all work so that it's easy to follow and understand. If 2.35 g of Cuso, is dissolved in 0.51 x 102mL of 0.380 M NH3, calculate the concentrations of the following species at equilibrium. x 10M Enter your answer in scientific notation. NH3 Cu(NH3)22+
Be sure to answer all parts. The equilibrium constant Kc for the reaction I2(g) ⇆ 2I(g) is 3.84 × 10−5 at 724 ° C. Calculate Kc and KP for the equilibrium 2I(g) ⇆ I2(g) at the same temperature. Kc = × 10 (Enter your answer in scientific notation.) KP =
Be sure to answer all parts. A 0.1276 sample of a monoprotic acid (molar mass = 1.10 x 10 g/mol) was dissolved in 25.0 mL of water and titrated with 0.0633 M NaOH. After 10.0 mL of base had been added, the pH was determined to be 5.67. What is the K, for the acid? x 10 (Enter your answer in scientific notation.)
Be sure to answer all parts. At 1130°C, the equilibrium constant (K) for the reaction 2H2S(g) = 2H2(8) + S2(8) is 2.25 x 10-4. If [H2S] =5.10 x 10-3 M and [H2]=1.30 10-3 M, calculate [S2]. x 10 M (Enter your answer in scientific notation.)
Be sure to answer all parts. At 1130°C, the equilibrium constant (K) for the reaction 2H,S(g) =2H2(g) +S2(8) is 2.25 x 104. If [H,8] = 4.50 x 10-2 Mand [H2] = 1.50 10-M, calculate [S2]. * 10 M (Enter your answer in scientific notation.)