(a) Write balanced molecular equations for the following potential precipitation reactions. Indicate the states of reactants and products [(aq) or…

1.(a) Write balanced molecular equations for the following potential precipitation reactions. Indicate the states of reactants and products [(aq) or (s)]. (b) In those cases where a precipitate forms, write the net ionic equation. If there is no reaction, state “No reaction.”
(i) CoCl2 (aq) + K2S (aq) → (ii) NaCl (aq) + (NH4)2S (aq) →
(iii) (NH4)2SO4 (aq) + Ba(NO3)2 (aq) → (iv) CuCl2 (aq) + K2S (aq) →  
2. Each of the following salts can be prepared from an acid and a base. Write the balanced molecular equation and the net ionic equation for the preparation of each. Indicate states of the reactants and products [(aq), (s), (l)]. Review solubility rules if necessary to determine the solubility of the reactants. (a) KClO4 (aq) (b) Cs2HPO4 (aq) (c) Ca(NO3)2 (aq)  
3. Assume that 3.3872 g of Na4SiO4 is dissolved in enough water to make 100.0 mL of solution. (a) What is the molarity of Na4SiO4? (b) What is the molarity of the sodium cation? (c) What is the molarity of the silicate anion? The molar mass of Na4SiO4 is 184.042 g/mol. 
4. You have a solution of 0.1127 M calcium chloride. (a) How many moles of solute are contained in 27.85 mL of solution? (b) How many grams of solute are contained in 27.85 mL of solution? (c) What volume (in millilitres) of solution is needed to obtain 0.00650 moles of solute? 
5.Suppose you need 2.50 L of 1.60 M sulfuric acid, but only the concentrated acid (17.8 M) is available. What volume (in L) of the concentrated acid must you dilute to 2.50 L to obtain 1.60 M sulfuric acid?
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