Write the net ionic equation, including phases, that corresponds to the reaction Zn(NO, ),(aq) + Na,Co,(aq)ZNCO,(s) + 2 NANO, (aq) net ionic equation:

Balance the following equation, classify the reaction as combination, decomposition, single displacement, or double displacement, and write the total ionic equation and net ionic equation.

A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required.    The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s)    How many moles of Ag+ (aq) ions are used to reach the end point?    How many moles of Cℓ- (aq) have reacted in the titration?    How many grams of chloride are present in the sample?   What is the mass percent of chloride in the sample?

The reaction of hypothetical elements: A, B, C, D, and E, follows the molecular equation:   AB2(aq) + CDE(aq) -> AE(s) + CB(aq) + DB(aq)   Assuming that all aqueous compounds would fully dissociate, indicate the element/s that would form spectator ions in the subsequent total ionic equation.

Use the activity series to predict which of the following reactions will occur. Complete and balance the equations. If no reaction occurs, write “no reaction” as the product. (a) Cu(s) + NiCl2(aq) ------> (b) Rb(s) + H2O(l) ------> (c) I2(s) + CaCl2(aq) ------>

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) Na₂S (aq) + Pb(NO3)2 (aq) → (iii) MgCl₂ (aq) + Pb(NO3)2 (aq) → (ii) FeSO4 (aq) + Na3PO4 (aq) → (iv) K₂SO4 (aq) + Ni(NO3)2 (aq) →

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The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,O, (aq) (thiosulfate ion). The determination is based on the net ionic equation 2 S,0 (aq) + 1, (aq) → S,0 (aq) + 31-(aq) Given that it requires 38.6 mL of 0.470 M Na, S,O, (aq) to titrate a 10.0 mL sample of I, (aq), calculate the molarity of I, (aq) in the solution. [5] = M

How much water (in mL) should you add to 50.0 mL of 0.300 M H,SO, (ag) to get a solution of 0.130 M H2SO4 (aq)? Write just the numerical answer with proper sig figs (no units) and do not put it in scientific notation. Make sure to record and submit the full work with units and sig figs in the separate file labeled 4 work.