Use the solubility rules to predict whether the following compounds are soluble AgCl PbSO4 CaCl2 Choose... ✓ Choose... water insoluble water-soluble → water?
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- Dilute sodium cyanide solution is slowly dripped into a slowly stirred silver nitrate solution. A white precipitate forms temporarily but dissolves as the addition of sodium cyanide continues. Use chemical equations to explain this observation. Silver cyanide is similar to silver chloride- in its solubility.Is AgC2H3O2 soluble in water? The solubility rules are leading me to believe it is, given Ag is a cation and all cations are soluble when combined with C2H3O2. Is this assumption correct?Predict the solubility and explain why: a) CdCO3 b) Na2S c) PbSO4 d) (NH4)3PO4 e) Hg2Cl2
- 25c. At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0068 M. You have found Ksp to be 1.6 × 10⁻⁹. If solid In₂(SO₄)₃ is added to a solution that already contains 0.150 M In(NO₃)₃, what will the new solubility of the solid be?During our Laboratory session for Organic chemistry, we were tasked to do a Bromine's test for hydrocarbons. We used 2% Br in CCl4. The samples were: A. Kerosene B. Heptane C. Toluene D. Xylene E. Unknown F. Corn Oil The result is shown in the attached picture. Based on other references, the result should either be a colorless or an orange/brownish solution. However, based on our result, there seems to be a formation of other compounds in some samples. My question is, what is the yellow precipitate-like product in sample A when Bromine was added and the yellow layer at the top of sample F? Could you give the different chemical equations that show the reaction in each sample when Br is added?A comparative analysis of organic compounds were done on various unknown samples labelled as A, G, N, U, Y. After multiple solubility tests, the following observations were recorded: I. Sample G dissolved in water and produced litmus paper results: Red → Red; Blue → Red II. Sample A did not dissolve in water, but dissolved in aq. HCl. III. Sample N did not dissolve in water, but dissolved in aq. NaOH. Further testing confirmed that it is insoluble in aq. NaHCO3. IV. Sample Y dissolved in water and produced litmus paper results: Red → Blue; Blue → Blue V. Sample U is insoluble in H2O, aq. NaOH, aq. HCl and concentrated H2SO4. What is the most probable identity of sample G? What is the most probable identity of sample A? What is the most probable identity…
- A comparative analysis of organic compounds were done on various unknown samples labelled as A, G, N, U, Y. After multiple solubility tests, the following observations were recorded: I. Sample G dissolved in water and produced litmus paper results: Red → Red; Blue → Red II. Sample A did not dissolve in water, but dissolved in aq. HCl. III. Sample N did not dissolve in water, but dissolved in aq. NaOH. Further testing confirmed that it is insoluble in aq. NaHCO3. IV. Sample Y dissolved in water and produced litmus paper results: Red → Blue; Blue → Blue V. Sample U is insoluble in H2O, aq. NaOH, aq. HCl and concentrated H2SO4. What is the most probable identity of sample G? What is the most probable identity of sample A? What is the most probable identity…Why is carbon chemistry clearly complex?Silver carbonate has a Ksp = 6.26×10-11 and a solubility of 0.0002501 M in water. Solid silver carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×10-10 M?
- Atmospheric Carbon dioxide is increasing. What effect does this have on coccolithophores and why? Your question should discuss each step in the inorganic carbon cycle discussed in class and should specifically address the effect of increased atmospheric CO2 on ocean pH.A solution is prepared by dissolving 0.090 g of PbI2 in 1.00 L of hot water and cooling the solution to 25°C. Will solid precipitate result from this process, according to the solubility product expression? Explain.Assign reasons for the following :(i) Transition metals and many of their compounds act as good catalysts.(ii) Transition metals generally form coloured compounds.