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#1. (2 marks x5 10 total) The following statements all relate to this redox reaction, which occurs in acidic solution: Unbalanced: Fe?-(aq) Cr2Oz?-(aq) Fe?-(aq) Cri...

Question

#1. (2 marks x5 10 total) The following statements all relate to this redox reaction, which occurs in acidic solution: Unbalanced: Fe?-(aq) Cr2Oz?-(aq) Fe?-(aq) Cri-(aq) Identify the following statements as true or false, AND give a reason why (a fewkey words)_ T / F The oxidation state of Cr in Cr2Oz2 anion is +VI:T / F The oxidizing agent is Fe?+ and the reducing agent is Cr2Oz2T / F In order for this reaction to happen , 3 electrons must be transferred in total.T / F In order for this reactio

#1. (2 marks x5 10 total) The following statements all relate to this redox reaction, which occurs in acidic solution: Unbalanced: Fe?-(aq) Cr2Oz?-(aq) Fe?-(aq) Cri-(aq) Identify the following statements as true or false, AND give a reason why (a fewkey words)_ T / F The oxidation state of Cr in Cr2Oz2 anion is +VI: T / F The oxidizing agent is Fe?+ and the reducing agent is Cr2Oz2 T / F In order for this reaction to happen , 3 electrons must be transferred in total. T / F In order for this reaction to happen, 6x as many moles of Fe?+ will be used relative to the Cr20z2 used: T / F In order for this reaction to happen; Ht must be consumed and HzO must be produced: #2. (10 marks) Black-and-white photographic film contains silver salts, and after developing the film, the used developing solution contains dissolved Ag" ions. The valuable silver ions can be recovered from this solution by precipitating them out as insoluble AgCI(s). If you treat a 100.0 mL solution containing 0.20 M AgNOz with 100.0 mL of 0.15 M CaClz, what mass of AgCl(s) will be formed? Will all the silver ions be removed from the solution?



Answers

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid-base, or oxidation-reduction. a. $\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{KNO}_{3}(a q)$ b. $\mathrm{HCl}(a q)+\mathrm{Zn}(s) \rightarrow \mathrm{H}_{2}(g)+\mathrm{ZnCl}_{2}(a q)$ c. $\mathrm{HCl}(a q)+\mathrm{AgNO}_{3}(a q) \rightarrow \mathrm{HNO}_{3}(a q)+\mathrm{AgCl}(s)$ d. $\mathrm{HCl}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{KCl}(a q)$ e. $\mathrm{Zn}(s)+\mathrm{CuSO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{Cu}(s)$ f. $\mathrm{NaH}_{2} \mathrm{PO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{Na}_{3} \mathrm{PO}_{4}(a q)+$ $\mathrm{H}_{2} \mathrm{O}(l)$ $\mathrm{g} \cdot \mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{CaSO}_{4}(s)+\mathrm{H}_{2} \mathrm{O}(l)$ h. $\mathrm{ZnCl}_{2}(a q)+\mathrm{Mg}(s) \rightarrow \mathrm{Zn}(s)+\mathrm{MgCl}_{2}(a q)$ i. $\mathrm{BaCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{HCl}(a q)$

So here we have a series of unbalanced equations and were identifying them to belong with precipitation reaction acid or base or Redux. So the different types of reactivity that we've got going on in all of these examples through the first example, we have a So this forms B A S O. For in the solid state, there's a precipitation reaction because we have that solid. Next, we have a Redox reaction that is B because what we have is CNN gives us c n two plus add two electrons and to H plus add two electrons. Gives us a church, too. You can see that Redux reactivity. In the third example, we have a precipitation reaction again, Part C. Because we have a G C L. There's a solid that forms. Next, we have an acid base reaction because we have a double displacement. So we essentially cr CR minus and r O H minus switch partners. So we formed h 20 k. C. L. Next we have in Redox reaction part E f is an acid base. G is an acid base. Again, H, we see is an oxidation reduction reaction. All right, it's precipitation. The reasons that we've already previously discussed

So here we have loads of reactions that we can look at and we are identifying whether there precipitation, reactions, acid or base or Redux. So the first example we have is a Redox reaction. Second example, we see is also considered a redox reaction because we see the transfer of electrons in the thought example we have seat. This is an acid base reaction. This is also considered a double displacement because s 04 to minus and ohh essentially switch partners. But with D, we have an acid base reaction. But it is also a precipitation reaction because we form a solid product at the end with a. This is an example of a precipitation reaction because we form a solid product that is insoluble in water with F. We have a precipitation reaction again with forming a solid that's insoluble in water. With G, we have an oxidation reduction reaction. Could we have the transfer of electrons with age? We have an oxidation reduction reaction because again we have the transfer of electrons with I, we have an acid base reaction. So this is also considered a double displacement reaction because the anti on CH minus and there are no three miners are exchanged

Here we are identifying each of the unbalanced reactions as either Precipitation Asset Base or Redux things First. Example. We have part A. That is a reduction reaction because we have the transfer of electrons. B. This is an acid base because we have the presence of the acids and bases within the chemical reactivity. So part C. There's an oxidation reduction reaction. You have the transfer of electrons party. This is an acid base reaction. E can take a look at next. So this is a precipitation reaction. So when we have a precipitation reaction, we're forming a solid product. And then f is also a precipitation reaction because we're forming a solid product. Next, we're looking at G, so this is an acid base Reaction. H is a precipitation reaction again with forming a solid product, and I is an oxidation reduction reactions

This question asks you to identify the following reactions as oxidation reduction, acid base or precipitation reaction. It's going to be an oxidation reduction reaction if we have a change in charge. Here we have oxygen with a Tu minus charge, going to oxygen with no charge. So this is an oxidation reduction reaction, and we have sulfuric acid reacting with copper. Here we have copper going from no charge to two plus. So another oxidation reduction reaction. When sulfuric acid reacts with sodium hydroxide producing the salt, sodium hydroxide and water, it's an acid base reaction. Any time we produce a salt and water, said acid based reaction, then we have sulfuric acid reacting with barium hydroxide, producing a solid. Anytime we produced a solid in an acquis environment, this would be a precipitation reaction. But because we are also producing a salt and water, it's an acid base reaction. So it's both acid base and precipitation. We have silver nitrate reacting with copper to chloride producing copper to nitrate and silver chloride, silver chloride being the solid. Anytime we produce a solid and iniquitous environment, it's a precipitation reaction. Then we have potassium hydroxide reacting with copper. Two sulphate producing copper to hydroxide solid and potassium sulfate. Again, a solid is formed, so it's a precipitation reaction. Fergie. We have chlorine gas reacting with Florian producing chlorine fluoride because each of these have a change in charge, going from no charge to a one plus and a one minus. It's an oxidation reduction reaction for H. We have no plus O two goes to know to. Here we have oxygen with no charge going to an oxygen with the Tu minus charge. So it's an oxidation reduction reaction and then calcium hydroxide reacting with nitric acid producing calcium nitrate, which is assault and water, would be an acid based reaction. Salt and water is the product as to base reaction.


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