Formula of tetrachlorocuprate(II) = [CuCl4]2-
Balanced equation :
[CuCl4]2-(aq) + 2 OH-(aq)
Cu(OH)2(s, blue) + 4 Cl-(aq)
Balanced equation :
Cu(OH)2(s)
CuO(s) + H2O(g)
Balanced equation :
2 [CuCl4]2-(aq, green) +
[Fe(CN)6]4-(aq, yellow)
Cu2Fe(CN)6(s,maroon) + 8
Cl-(aq)
Oxalate ion will interfere with the Group D tests after we make the solution acidic. Also,...
We separate the iron hydroxide ppt from the supernatant liquid containing the aluminum complex ion by centrifuging the reaction mixture and decanting the supernatant liquid. We verify the presence of iron ion in the hydroxide ppt by dissolving the iron (I) hydroxide in a minimal amount of aqueous HC forming yellow [FeCla] Write the reaction described above including phases Adding yellow potassium ferrocyanide solution, KaFe(CN)s, causing formation of a solid dark blue dye, iron () hexacyanoferrate (), Fea[Fe(CN)s]3, known as...
Aluminum ion in solution reacts with water to form aqueous hexaaguaaluminum ()ion. Write this reaction below, remember phases. Aluminum is more likely to form a hydrated complex than the other four ions remaining in solution, because of its relatively small size and high charge To separate the Group B2 ion, the solution first is made basic by adding ammonia. In the presence of this weak base the pH is adjusted to 9-10 and the group B ions form insoluble hydroxides....
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2. Give chemical equations for the following: a. Precipitating the silver ion by adding hydrochloric acid b. Precipitating the copper ion by adding sodium sulfide c. Dissolving the copper sulfide in concentrated nitric acid to precipitate sulfur. (The orange gas that you saw is NO, product, and sulfur precipitate can be shown as "S") d. Confirming the identity of the ion as copper by adding potassium ferricyanide. (Pote is only a spectator ion...
Identifying the Group E ion potassium The supernatant liquid remaining after the copper (11) hydroxide separation contains the potassium ion. Add acetic acid to make the pH of the solution 4-5. Add sodium bexanikuitecebaltat (l) solution Na:CoNOG or sodium cobaltinitrite. The resultinformation of a yellow precipitate of potassium cobaltinitrite, K-CoNOa)s indicates the presence of potassium ion. x 18e)+ Co/NO:]alles, yellow) + K.Ca(NO)els, yellow)
1.A solution contains 1.09×10-2 M potassium carbonate and 1.36×10-2 M ammonium sulfide. Solid copper(II) acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu2+] = M 2. A solution contains 6.93×10-3 M cobalt(II) nitrate and 1.32×10-2 M zinc acetate. Solid potassium carbonate is added slowly to this mixture. A. What is the formula of the substance that...
A solution contains 1.01×10-2 M potassium hydroxide and 6.56×10-3 M sodium sulfide. Solid copper(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? Formula= B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu2+] = ___M
If we have 50 mL of a 1.0M sodium hydroxide solution and 50 mL of a 0.20 M iron (III) nitrate solution, what is the concentration of ions in each solution? Write the chemical, complete ionic and net ionic equations for the reaction. Chemical: Complete lonic: Net Ionic: What volume of 1.0M NaOH is required to precipitate all the Fe ions from 50. mL of a 0.20 M Fe(NO) solution? What mass of iron (II) hydroxide precipitate can be produced...
Chemical Reactions For each reaction you observed, the names of the reactants and products are given below. You must: 1. Write the correct formula for each reactant and product. Balance each equation. 2. A. Combination reactions magnesium oxide 1. Magnesium + oxygen (unbalanced) Mg+ O, MgO sulfur dioxide 2. Sulfur + oxygen B. Analysis of the Copper Content of a Penny po zinc chloride + hydrogen zinc + hydrochloric acid HCI ZnCl, 1. (unbalanced) н, Zn + C. Single Replacement...
Need help for
answering first part(1) color change is due to presence? And what
was the reason for the equilibrium turn to reverse direction? And
also last 2 questions.!
Chemistry 102 EXPERİMENT3 Equilibrium& Le Chatelier's Principle tive Qualita of this experiment is to study qualitative aspects of chemical systems in dynamic equilibrium. in doing this experiment, you will learm the operation of Le Chateliers principle. n Vslowly add 1 to 2 drops of dilute 6 M sodium hydroxide solution to...
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only need g, h and I please
Classifying Chemical Reactions continued Classifying Chemical Reactions continued 3. Write a balanced chemical equation for each reaction and classify the reaction. a. Copper metal heated with oxygen gives solid copper(II)oxide. 4 cu +02 → 2420 (5) combination reachon b. Mixing ammonium nitrate and sodium hydroxide solutions gives aqueous sodium nitrate, ammonia gas, and water. NHL NO2+ NaOH -> Na NO₃(aq) + NH₃ (9)+H₂O (e) double replacement c. Mercury(II) nitrate solution reacts with...