one reaction should be selected in each of the following four categories: (a) acid base reactions, (b) complex ion reactions, (c) gas forming reactions and (d) precipitation reactions. For each reaction write a balanced chemical reaction including physical states [solid (s), liquid (ℓ), gas (g) or aqueous solution (aq)]. Net ionic reaction equations are preferred, but not required. For example, the reaction of nickel(II) chloride and ammonium hydroxide could be written in either of the following ways:

Predict the products of each precipitation reaction, listing the solid precipitate first, and then balance the completed equation. (Enter your answers using the format CH4 for CH. Use the lowest possible coefficients.) (s)+[ (a) (aq) (b) Ca(NO3)2(aq) + Na,C,04(aq) → Pb(NO3)2(aq) + KBr(aq) → ](s) + C (aq)

The following reaction occurs when two aqueous solutions are mixed: Cr(NO3)3(aq) + 3NaOH(aq)   → Cr(OH)3(s) + 2NaNO3(aq) Identify the spectator ion OR ions in the solution. SELECT ALL SPECTATOR IONS!

Predicting the reactants of a neutralization reaction Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. [] → NaCIO_(aq) + H,O) H₂O(1) X 1/5 Ś ? oll 18 Ar A. For efloor

write the net ionic equation for the reaction in the photo

A student Investigated the stoichiometry of the reaction of zinc (Zn) and HCl solution and reported the following data. When 0.2158 g of Zn reacted with 10.00 ml of 1.000M HCl, 82.062 g of water was displaced. A total of 36.00 ml of 9.501 x 10-2M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. Calculate the volume of the displaced water from its mass (which will be equal to the volume of the gas collected.) 2) Calculate the pressure of the H2 collected 3) Calculate the number of moles of H2 collected using the ideal gas equation. 4)calculate the number of moles of hcl remaining in the flask at the end of the reaction 5) caluxukage the number of miles of hcl originally present in the reaction  6) calculate the number of moles hcl reacting  7) ccalculate the number of moles zn reacting 8) calculate the ratio of the number of hcl reacting to the number of…

The concentration of SO42– ions in a 45.0 mL sample of seawater is determined by adding a solution of BaCl2 and precipitating the SO42– as BaSO4. After the precipitate is filtered from the solution, it is dried and weighed. If the mass of BaSO4 recovered is 0.315 g, what is the sulfate concentration of the seawater sample? Express your answer in mmol/L.

Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HC1), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HC1 through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(1) + CO₂(g) The CO₂ gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 150. mL of a 0.010 M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl ? Round your answer to 2 significant digits. ■ x10 ×

1. (а) The solubility product of a sparingly soluble salt, XF2, was determined by titration and found to be 2.9 x 101º M. The procedure involved the following steps: (i) A saturated solution of the salt XF2 was prepared. (ii) 25.00 mL of this solution was titrated against a standardized 0.005 M HCl solution. Determine the titre value obtained in the experiment.

Write the net ionic equation for the following molecular equation. HBr is a strong electrolyte. CH3 COOH is a weak electrolyte. NaCH,COO(a) + нBr(aq) —+ NaBr(aq) + CH,COОҢ(аq) (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) +