Reaction of nickel carbonate and sulphuric acid?
You have to perform the experiment to make accurate observations. However, you can actually predict what would happen based on the reacting substances. You have a basic insoluble salt, nickel (II) carbonate and sulfuric acid. Based on the nature of the reactants, you can deduce that this is an acid base reaction (which is basically double displacement). Products are nickel (II) sulfate and carbonic acid. However, carbonic acid is unstable. This rapidly decomposes to carbon dioxide and water. So actual products of the reaction are nickel (II) sulfate, carbon dioxide and water. You would therefore, observe bubbling and disappearance of the nickel carbonate. Based on the solubility rules, the nickel (II) sulfate is soluble in water. So, you have to evaporate the water to recover it. You don't over evaporate the water because nickel (II) sulfate naturally exists as a hydrate and you have to answer question #5. The percent yield can only be calculated if you have the actual mass of the nickel (II) sulfate from the experiment. There are several sources of error that would make the % yield lower than expected. Again, performing the actual experiment helps a lot. However, one source of error is not letting the reaction go to completion (i.e. incomplete reaction between the reactants would result in less product formed). Another is losing some of the nickel (II) sulfate through spillage of the solution or during transfer from one container to another.
What is the reaction to form (NH4)2Ni(SO4)2*xH2O (Ammonium Nickel Sulfate Hydrate)?
nickel ammonium sulfate is a double salt, Ni(NH4)2(SO4)2.6H2O or NiSO4. (NH4)2SO4. 6H2O The reaction to form it would be to dissolve one mole of nickel sulfate in water , and 1 mole of ammonium sulphate in water in a second container. You simply mix then crystallise. specific details of a lab method are given below that contains concentrations that will crystallise spontaneously: Lab prep of Ammonium nickel sulfate, (NH4)2 SO4. NiSO4.6H2O Measure 2.0 mL of saturated nickel chloride solution into a small flask or beaker, and dilute it with an equal volume (2.0 mL) of purified water. Measure 5.9 mL of saturated ammonium sulfate solution into a small flask or beaker, and dilute it with an equal volume (5.9 mL) of purified water. If either solution contains suspended insoluble impurities, filter it. Pour both solutions together into a crystallising dish, cover the dish with a light dust cover (a filter paper is suitable) and let it stand. At a room temperature of about 25oC, crystallisation should commence within about ten minutes, and be advanced within about one to one and a half hours. Drain off the (pale green) supernatant solution, scrape the crystals onto a small wad of dry filter paper and sponge them dry. The colour of the residual supernatant solution should be very pale green, indicating that the amount of nickel being discarded with the supernatant solution is very small. The yield from this preparation should be close to 90% of the theoretical maximum.
How to prepare1000 ppm nickel standard solution using nickel sulfate ?
If you are using reagent grade Nickel Sulfate, you will first need to identify if you have a hydrated standard or not. Nickel Sulfate is available in non-hydrated form: NiSO4 and in the hydrates NiSO4*6H2O or NiSO4*7H2O. Formula weights: Ni = 58.6900 g/mol NiSO4 = 154.7536 g/mol NiSO4*6H2O = 262.8448 g/mol NiSO4*7H2O = 280.8600 g/mol 1000 ppm is the same as writing 1000 mg/L. So you want 1000 mg Ni in every 1 L of solution, which is 1.000 g/L. I will assume you are making exactly 1 liter of solution. If you have unhydrated NiSO4, then the math looks like this: X g NiSO4 * (58.6900 g Ni / 154.7536 g NiSO4) = 1.000 g Ni X = 2.6368g NiSO4 If you have the hydrate, NiSO4*6H2O: X g NiSO4*6H2O * (58.6900 g Ni / 262.8448 g NiSO4) = 1.000 g Ni X = 4.4785g NiSO4*6H2O And for the hydrate, NiSO4*7H2O: X g NiSO4*7H2O * (58.6900 g Ni / 280.8600 g NiSO4) = 1.000 g Ni X = 4.7855 g NiSO4*7H2O
Why do we use sulfuric acid in the preparation of nickel ammonium sulphate?
The obvious answer is not so obvious. Suppose we have nickel sulfate and ammonium sulfate as starting reagents. We mix these in solution in the right stoichiometric ratio of 1 mole of ammonium sulfate ((NH4)2SO4) to one mole of nickel sulfate (Ni2SO4). We want the double salt and not the metal ammine. With no acid added there will be a certain amount of ammonia in solution which will tend to form the set of complex ions Ni(NH3)x(H2O)6-x We do not want this contaminant. To make sure that all of the ammonia is converted to ammonium (NH4+) we add sulfuric acid. This also makes the crystals form best. I know because I have made such crystals.
What happens when: concentrated ammonia solution is added to nickel (II) sulfate solution?
NiSO4(aq) & 6 NH3(aq) --> {Ni (NH3)6]+2 (aq) & (SO4)-2(aq) nickel can form a complex with 4 NH3 "s . but 6 is more common as prepared in normal qualitative analysis procedures: http://74.125.155.132/search?q=cache:bxh... had you added dilute NH3 it would have formed the precipitate NiOH)2
Why does a nickel spatula cannot be used to the stir solution of a copper sulfate solution?
Why does a nickel spatula cannot be used to the stir solution of a copper sulfate solution?First, check your typing before posting. The text of this homework question* surely did not have three errors in its original wording.(It was likely something close to “Why is it that a nickel spatula cannot be used to stir a copper sulfate solution?”)Next, go read about single-displacement reactions—here, or maybe even in your chemistry textbook—and the reactivity series.Easy research can give easy answers.*Don’t post homework questions here. You are supposed to learn from your work.
Calculate the mass of nickel(II) sulfate and the mass of water contained in 200. g of a 6% solution of nickel?
Calculate the mass of nickel(II) sulfate and the mass of water contained in 200. g of a 6% solution of nickel (II) sulfate. Please help! Show the work you did to come to the answer. Thank you!
What is the chemical reaction of zinc and copper (II) sulfate?
Explanation -Zinc is more reactive than copper. So, here , on adding zinc to CuSO4 solution, zinc displaces copper from copper sulphate & forms zinc sulphate solution. This is indicated by colour change from blue to colourless. CuSO4 solution has a blue colour while ZnSO4 solution is colourless. Chemical equation -Zn(s) + CuSO4(aq) -> Cu(s) + ZnSO4 (aq).Type of reaction -It's a displacement reaction.It's a redox reaction. Oxidation number of Cu decreases from 2 to 0 so it's reduced. Oxidation number of Zn increases from 0 to 2 so it's oxidised.
Concentration solution problem...? need help...?
The amount of the substance (total weight minus the water contributed by the hydrate) is 2402 - 987.9 = 1414.1 g. If we add "x" g of water to make a 25% solution, the new total weight would be x + 2402. Therefore concentration = 0.25 = 1414.1/(x + 2402) 0.25x + 0.25* 2402 = 1414.1 x = (1414.1 - 0.25* 2402)/0.25 x = 3254.4 g
What is nickel dimethyl glyoxime? What is the procedure to prepare it in laboratory?
From the Wikipedia article on Dimethylglyoxime: "Dimethylglyoxime (dmgH2) is used as a chelating agent in the gravimetric analysis of nickel. The use of DMG as a reagent to detect nickel was discovered by L. A. Chugaev in 1905. For qualitative analysis, dmgH2 is often used as a solution in ethanol. It is the conjugate base, not dmgH2 itself, that forms the complexes. Furthermore, a pair of dmgH(1-) ligands are joined through hydrogen bonds to give a macrocyclic ligand. The most famous complex is the bright red Ni(dmgH)2, formed by treatment of Ni(II) sources with dmgH2. This planar complex is very poorly soluble and so precipitates from solution. This method is used for the gravimetric determination of nickel, e.g. in ores. The color of the precipitate is red."