(a) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M NH3? NH3(aq) + HCN(aq) ⇒ NH4+ (aq) + CN ¯(aq) Kc = 0.71 M 4.0 (b) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M K₂S? S² (aq) + HCN(aq) = HS¯(aq) + CN −(aq) Kc = 3.1 x 10³ 5.0e2 XM 4.0
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- According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?Suppose 234.3 mg of PbCl2 was added to 16.0 mL of water in a flask, and the solution was allowed to reach equilibrium at 21.0 oC. Some solute remained at the bottom of the flask after equilibrium, and the solution was filtered to collect the remaining PbCl2, which had a mass of 91.6 mg . What is the solubility of PbCl2 (in g/L)? -Express the concentration in grams per liter to three significant figures.Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed. (a) What is the molar solubility of BaSO4? (b) What is its solubility in grams per 100 g of water?
- 1. What is the balanced net ionic equation for the equilibrium involving the solutbility o Mg (OH)2? 2. When heating the mixture it had no color and the reaction was declared endothermic. Is the forward reaction endothermic or exothermic and why? What is the balanced net ionic equation when heat is included? 3. Most solids are more soluable in warm water than cold water. Does the soluability of Mg (OH)2 fit this pattern? Why?In a titration of Vinegar, the average volume of 0.1 M NaOH used after three titrations is 4.26 mL. If the density of vinegar (acetic acid) is 1.006 g/ml and the molecular mass of CH3COOH is 60.05 g/mol. The mass percent (%m/v) of the vinegar is: 5x10-5 5x10-4 0.5 5x10-3Suppose a 0.25 M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium molarity of HPO4 2−. You'll find information on the properties of phosphoric acid in the ALEKS Data resource. Round your answer to 2 significant digits.
- Consider this reaction equation: A2B(g)= 2 A(g) + B(g) If you start with 1.2 M A2B, and if at equilibrium, 50% of it has decomposed, what are the equilibrium concentrations of A and B? What is the value of the equilibrium constant?When HCl(aq) is added to calclum carbonate solid, carbon dioxide gas, liquid water and aqueous calcium chloride form: Caco,(s) + 2HCI(aq) - CO,lg) • CaCl, faq) + H,00) This reaction is used by geologists to confirm the presence of limestone (calcium carbonate) in minerals. In this experiment you are trying to determine the effect of concentration of HCI(aq) on the production of carbon dioxide. a. Based upon the information above, come up with a question to answer. (C:1) You can use the following equipment to answer this question: calcium carbonate chips, 1.90 molL HClaq). pH meter (measures hydrogen ion concentration), beaker, timer, apparatus to measure gas produced b. Based upon the equipment provided above, design a procedure to answer your question. Ensure you provide numbered steps. (1:3, C:2) c. Hypothesize an answer to your question. (I:1) Give reasons for your hypothesis. Ensure you are very specific. (A3) From your experiment, you collect the following data: Reactant…The solubility product for Mg3(PO4)2 is 6.3 x 10‒26. What is the solubility of Mg3(PO4)2 in pure water, in grams per liter?
- You choose to investigate some of the solubility guidelinesfor two ions , the chromate ion(CrO4)-2 and the oxalate ion (C2O4) - 2. You are given 0.01 Msolutions (A, B, C, D) of four water-soluble salts: When these solutions are mixed, the following observationsare made as given in table: (a) Write a net ionic equation for the reaction that occurs ineach of the experiments. (b) Identify the precipitate formed,if any, in each of the experiments.Consider the following equilibrium: Cu2+(aq)+ 4NH3(aq) ⇌ Cu(NH3)42+(aq); Kf= 1.7 x 1013; Determine [Cu2+], [Cu(NH3)42+], [NH3],and [SO42–], respectively, in solution that results from mixing 20.0-mL solution of 0.10 MCuSO4and a 30.0-mL solution of 3.0 M NH3 are mixed.Please write the complete ionic equation when mixing the following two aqueous salts: P b ( N O 3 ) 2 ( a q ) + K I ( a q ) ⟶ ??? ***All chemical equations must be balanced, have proper subscripts/superscripts, and list the state of the chemical***