8. Complete the following precipitation or acid/base reactions with balanced total ionic equations: 3 CaCl₂ + 2 CS3PO4 Ba(OH)₂+ FeSO4->BaSO4 + Fe²+ + 2OH Ca(OH)2 + 2 CH3COOH KOH+HI->

Write a balanced net ionic equation. If no reaction occurs, write the products exactly as the reactants are written and all coefficients are 1. Ag+ + Cu

You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?

A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.

A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The titration of this solution with a KOH solution requires 20.50 mL of the base (KOH solution) to reach the “end-point”. What is the molar concentration of KOH solution? The reaction occurs as follows:                       KOH(aq)  +  KHC8H4O4(aq)  -->  K2C8H4O4(aq)  +  H2O(l)           (A) 0.2457 M           (B) 0.1315 M           (C) 0.05390 M           (D) 0.03823 M

Write a balanced molecular equation for the reaction that occurs when aqueous solutions of sodium hydroxide, NaOH, and hydrochloric acid, HCl, are combined. It is not necessary to include states such as (aq) or (g). + +

An aqueous solution of Ca(OH)2with a concentration of 0.188 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid?

Predict the products and balance the following reaction, write a complete ionic equation, and a net ionic equation. What type of reaction is this? AgNO3 + K2CO3  -->

Complete and balance gas-evolution equation. HC2H3O2(aq) + NaHSO3(aq) ------>

2Fe(s) + 3Cu2+(aq)  2Fe3+(aq) + 3Cu(s) a)Calculate the minimum volume of 1.16M CuSO4 solution that is required to ensure complete reaction of 1.04g of Fe.Since you do not know which reaction will be the one to occur, you must base the calculation on whichever of the equations requires more CuSO4 solution. b)To ensure that sufficient CuSO4 is used, it is common practice to add an excess.Calculate the volume of 1.16M CuSO4 needed to provide a 20% excess in this case.