what is the concentration of K+ in 0.15 M of K2S
What is the concentration of K+ in 0.15 M of K2S? If CaCl2 is dissolved in water, what can be said about the concentration of the Ca2+ ion? It has the same concentration as the Cl− ion. Its concentration is half that of the Cl− ion. Its concentration is twice that of the Cl− ion. Its concentration is one-third that of the Cl− ion. A scientist wants to make a solution of tribasic sodium phosphate, Na3PO4, for a laboratory experiment....
Part A: What is the concentration of K^+ in 0.15 M of K2S ? Part B: If is dissolved in water, what can be said about the concentration of the ion? It has the same concentration as the ion. Its concentration is half that of the ion. Its concentration is twice that of the ion. Its concentration is one-third that of the ion. Part C: A scientist wants to make a solution of tribasic sodium phosphate, , for a laboratory...
what is the concentration of K+ in 0.15M of K2S
Calculate the equilibrium concentration of Ni?that is 0.05 M in potassium hydrogen phthalate, KHP, and 0.15 M in potassium phthalate, KP. Phthalic acid: K 1 = 1.2x10-?; K 21 = 3.90x10
What is the equilibrium concentration of hydrogen ion in a solution of 0.15 M ammonia, NH3, Kb=1.8 × 10−5
Calculate the concentration of all species in a 0.15 M KF solution. Ka(HF)=6.3×10−4
Question 8. Suppose ZnS(s) is saturated with 0.04 M K2S (K2S completely dissolves and ZnS has limited solubility) (Ksp for ZnS is 2x10-25) (a) (2 pts) What is the ionic strength of the solution? Show calculations (b) (4 pts) What are the activity coefficients of each specie?(Please apply Debye Hückel equation given in lecture notes considering the size of the ion if necessary) (c) (4 pts) What is pZn by taking activity coefficients into consideration? Please show calculations
What is the pH of a 0.15 M solution of potassium nitrite (KNO2)? (K, value for HNO2 nitrous acid - 4.0 x 10-4) a. 11.43 d.5.71 b. 7.00 e. 11.89 c. 8.29 - -
What is the half-life for the decomposition of NOCl when the concentration of NOCl is 0.15 M? The rate constant for this first-order reaction is 4.75 x 10^-5 s^-1.
If the equilibrium concentration of each product is [0.035 M], and the equilibrium concentration of [HNO2] is 0.15, what is the equilibrium constant (K)? (please do not input answer using scientific notation). Based on the information given in the previous question, what is the pH of the solution?