Moving to another question will save this response. Question 2 What is the net ionic equation for the reaction of aqueous potassium hydroxide and aqueous magnesium chlori 1S K (aq) + OH (aq) KOH(s) КОНЕ) K*(aq) + Cl (aq) →KCI(s) Mg"(aq) + 2 CF (aq) MgCl2(s) 2+ o Mg-(aq)+3 OH (aq)Mg(0H)3(s) Mg-(aq) -2 OH (aq) Mg(OH)2(s) Me (aq) - Он (аq) — MgОН (9) MGOH (s A Moving to another question will save this response. search hp f11 f12 fg f10 f6 f7 f8 f4 f5 I미 & %24 4. 6. 7. 80 T. | 0O

Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom. oxidation state of highlighted atom species Na (aq) H30"(aq) co? (aq) Cl,(9)

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5

Write the net ionic equation, including phases, that corresponds to the reaction   Cu(NO3)2(aq)+K2S(aq)⟶CuS(s)+2KNO3(aq)

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s)  +   CuSO4 (aq)  →   Cu (s)  +   FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a  300.mL  copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of  67.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) – MnCl, (aq) + 2 H,0(1) + Cl, (g) > How much MnO, (s) should be added to excess HCl(aq) to obtain 105 mL Cl, (g) at 25 °C and 755 Torr? mass of MnO,:

When an ionic solid dissolves in water, water molecules attract the ions causing them to dissociate orcome apart. The resulting dissolved ions are electrically charged particles that allow the solution toconduct electricity. The following chemical equations represent this phenomenon:NaCl (s) → Na+ (aq) + Cl-(aq)Na2CO3 (s) → 2Na+(aq) + CO32- (aq)Write a similar balanced chemical equation for the other four strong electrolytes in the data table  NaHCO3 KNO3NH4Cl  HCl

[References] Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas ( CH4) by the following process: 2NH3 (g) + 30,(g) + 2CH, (g) →→ 2HCN(g) + 6H,0(g) Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reaction vessel contains 5.75 g NH3, 12.0 g 02, and 5.00 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written? Mass = HCN

a For the reaction СаBra (aq) + K,SO4 (ag) write the balanced formula equation. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) СаBr, (aq) K,SO,(aq) CaSO,(s) | 2KC1(aq)