For each of the following pairs of solutions, write a balanced molecular, total ionic, and net ionic equation. Include all physical states and ion charges!!! If no reaction is expected to occur, write “no reaction." 4. AGNO3 with KI Pb(NO;)2 with KI MGSO4 with NaC2H3O2 Na3PO4 with Ca(NO3) 2 MGSO4 with BaCl2 NHẠC1 with Ca(NO3)2 CoCl2 with Ca(OH) 2 А. В. С. D. Е. F. G.

Imagine the diagram shown below is a 'good representation' of a titration curve for the titration of 20.0 mL of 0.10 M Na4A with 0.15 M HCI. Use this information to fill in the blanks below. B A D. E pH F ●G H Volume of HCI (mL) a) Consider: A4(aq) + 2 H3O*(aq) → H2A² (aq) + 2 H20(1). This is the net ionic reaction that occurs between the beginning of the titration and to the equivalence point. b) After point along the titration curve the analyte is just starting to gain the 4th proton. (Type in A, B, C.) c) The point along the titration curve where concentrations of H2A2 and H3A are equal is (Type in A, B, C.) d) Molecules and ions: H4A, H3A", H2A², HA³- or A4- Of the molecule and ions shown above, the molecule or ion that

Assume the equivalent weight of an acid is 51.0.51.0. Calculate the number of mL of 0.233 M0.233 M NaOHNaOH that would be needed to titrate 0.466 g0.466 g of the acid.

3. Usin the Solubility predict whether a double displacement reaction will occur in each example below. If a reaction will occur, complete and balance the equation, properly indicating gases and precipitates. If you believe no reaction will occur, write "no side of the equation. All reactants are in aqueous solution. reaction" as the right-hand (а) K2S + CuSO4 (b) КОН + NH4CI (c) BiCl, + NaOH (d) NazCO3 + HNO3 (e) ZnBr, + K3PO4

Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). (suppose there is 1L of vinegar) 2. Use your average AA concentration to calculate the mass percent of acetic acid in vinegar. (suppose there is 1L of vinegar)

9. What is meant by a "dilute weak base? Provide an example. 10.U: e the data in Table 1 to answer the following Table 1: Titration Data Volume of magnesium hydroxide solution in Erlenmeyer flask Concentration of magnesium hydroxide solution in Erlenmeyer flask Initial volume of nitric acid solution in burette Final volume of nitric |acid solution in burette (7) Write the balanced chemical equation o) Calculate the molar concentration of nitric acid. marks) (c) Calculate the pH of the acid. 20.00 mL 0.135 mol/L 1.06 mL 23.08 mL Table 3 Solubility of Common lonic Compounds in Water Solubility of Compound Anion Mest 1. Mast Cation Alkali metal ions Li". K. Hb.. hydrogen in. H* Soluble Soluble Most ammoniam ion. NH; Soluble nitrate, NO, Mnt Soluble 2. ethanoate lacetate). CH,COO Lawe solubility Mast others Soluble chiloride, CI 3. bromide, Br ledide. Ag". P, Hg". Cu.n Low solutility All others Soluble Mg.C. a, P Loe sislutility Most others Soluble Ca, Se, Ba, Pb Low solulnility 5. mdtate,…

A 3.860 g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.30 mL of |0.796 M HCI, After treatment of the sample, some acid remains. If 28.0 mL of 0.118 M NaOH were required to titrate the excess hydrochloric acid, how many moles of sodium carbonate were present in the original sample? mol Na2 CO3 What is the percent composition of the original sample? % Na2 CO3 % NaCl

Lactic acid HC3H5O3 is a monoprotic acid that forms when milk sours. An 18.5 ml sample of a solution of lactic scid required 17.25 ml of 0.155M NaoH to reach an end point in a titration. (a) How many moles of lactic acid were in the sample? (b) how many grams of lactic acid were in the sample?

from that neede to titrate 25,0 mL of a 0.10 M HCI (a strong a solution? oblems 39 A quantity of 18.68 mL of a KOH solution is neede to neutralize 0.4218 g of KHP. What is the concen tration (in molarity) of the KOH solution? 4.98

5. Please Double check solution. Last 2 solutions have been completely wrong.