An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. Identify the solid in the balanced equation. A) (NH4 )2 SO4 B) Pb(NO3 )2 C) PbSO4 D) NH4 NO3 E) There is no solid formed when the two solutions are mixed. ____ 11. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride.
CHE 111 Laboratory 3 Hydrates Introduction Hydrates Water molecules combine with the molecules of certain substances, forming loose chemical combinations called hydrates. An example of a hydrate is MgSO4•7H2O. This formula means 7 water molecules are loosely attached to a magnesium sulfate molecule. Other examples of hydrates are Na2SO4•10H2O and Ba(OH)2•8H2O. When the hydrate is heated, it easily loses water molecules attached and becomes an anhydrous salt.
The chemical reaction used to find this constant is as follows: MgC2O4 (s) ↔Mg(aq)2++ C2O4 (aq)2- Kc= Mg2+[C2O42-][MgC2O4] Ksp=Mg2+[C2O42-] The solid salt magnesium oxalate is prepared through the following precipitation reaction: Mg(SO4)(aq)+NaC2O4 (aq) → MgC2O4 (s)+NaSO4 (aq) Next, the concentration of the Mg2+ and C2O42- ions is found through a redox titration. This redox titration uses a standardized potassium permanganate solution. The potassium permanganate solution is standardized by titrating it with samples of iron(II)ammonium sulfate hexahydrate . The end point is reached when the solution has turned light purple which is a result of excess amounts of MNO4-. This reaction can be summed up using the following formula: 5Fe2++8H++MnO4- →5Fe3++Mn2++4H2O After standardization, the potassium permanganate solution is then titrated with 3 different magnesium oxalate solutions.
The "salts" part of the name comes from their appearance being similar to the crystals of common salt. Chemically speaking, all bath salts are true salts but the more organic salts commonly used in bath water (especially surfactants like soap) are not called "bath salts" because those appear more like wax or oil instead. Such salts include magnesium sulfate (Epsom salts), sodium chloride (table salt), sodium bicarbonate (baking soda), sodium hexametaphosphate (Calgon, amorphous/glassy sodium metaphosphate), sodium sesquicarbonate, borax, and sodium citrate. Fragrances and colors are often added to bath salts; in fact, one purpose of salts is as a vehicle or diluent to extend fragrances which are otherwise too potent for convenient use. Other common additives to bath salts are oils (agglomerating the salts to form amorphous granules, the product being called "bath beads" or "bath oil beads"), foaming agents, and effervescent agents.
Test for Triiodide ion Triiodide is present if your tincture is a shade of orange or red-brown. The solution became an orange-red color which indicates that there is a good amount of triiodide ion present. Standards Test Positive Positive (contains Iodine) Positive Positive (contains Iodide and Chloride) Positive Positive (contains Triiodide) Focus Questions 1. How can I make a Pharmaceutical Product from Seaweed? First of all, a pharmaceutical product can be made from seaweed by heating seaweed in water.
Determination of a Solubility Product Abstract: The purpose of this experiment was to determine the solubility product constant (Ksp) for a sparingly soluble compound, Ca(OH)2, in pure water and in a NaOH solution. To determine the solubility product constant a solution of Ca(OH)2, in pure water was titrated with HCl. The concentrations of OH- and Ca2+ were used to calculate the solubility product constant. Another solution, containing Ca(OH)2, in NaOH was also titrated. The concentrations of OH- and Ca2+ were used to calculate the solubility product constant.
I believe we did our procedures accurately. The precipitate was Zinc hydroxide which is amphoteric in nature. Meaning it can react both with acid and base to form salt. We got a white precipitate of zinc hydroxide and it reacted to make salt with both the base sodium hydroxide and the acetic acid. Our result would have been clearer to observe if we centrifuged it long enough because we might have lost some of the precipitate while washing it since it was not centrifuged long enough.
3. Hypothesis: Iron (II) is going to be the reducing agent and that Mg is going to be the oxidizing agent. 4. Chart: Data Table: Solubility Rules Table | Negative Ion (Anions) | Positive Ions (Cations) | Solubility of Compound | All negative ion are _ with | Alkali ions | soluble | All negative ion are _ with | Hydrogen ion | Soluble | All negative ions are _ with | Ammonium ion | Soluble | Nitrate NO3 ions are _ with | Any cation | soluble | Acetate CH3COO ions are _ with | Any cation except Ag | soluble | Chloride, ClBromide, BrIodide, I | Ag+, Pb2+, Hg2+, Cu+, Tl+ | Low solubility | Sulfide, S | Ca2+, Sr2+, Ba2+, Ag2+,Pb2+, Hg2+ | Low solubility | 5. Materials: Cotton swabs, sheet of black and white paper, distilled water, goggles, well plate 24 & 96, pipet, Ionic Reactons bag 6.
This solution was placed in a burette and 18.4 cm3 was required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Deduce the molecular formula of the acid and hence the value of n. 5. Sodium carbonate exists in hydrated form, Na2CO3.xH2O, in the solid state. 3.5 g of a sodium carbonate sample was dissolved in water and the volume made up to 250 cm3. 25.0 cm3 of this solution was titrated against 0.1 moldm-3 HCl and 24.5 cm3 of the acid were required.