pipets (2) | |conductivity tester |CaCl2 (calcium chloride) | |ethanol |KI (potassium iodide) | |iron ring |NaCl (sodium chloride) | |ring stand |C13H18O2 (ibuprofen)
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water? Ksp = 6.0x10-27 for CdS. [ A: [ Q: ][ ] ][ ] ; ][ ] √ √ A solution in equilibrium with a precipitate of AgCl was found to contain 3.4x10-6M Cl . Calculate Ksp for AgCl. [ ( A: [ ][ ] ; ][ ] ) Q: Since the value of Ksp depends on the concentrations of the ions in solution‚ a larger value of Ksp indicates a more soluble salt‚ while a smaller value of Ksp indicates a less soluble salt. Which of the following salts is the most soluble? AgCl (Ksp = 1.8x10-10) AgI (Ksp = 8.5x10-17)
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analysis of ions present in a solution. A large industry that employs this type of chemistry is the mining industry. In the mining industry metals are not typically pure when first collected. Through the use of selective precipitation and the knowledge of Ksp values‚ certain metal ions can be precipitated out. EXPERIMENTAL The Selective Precipitation of the Barium Magnesium Group experiment instructions were followed directly from the handout printed from the course website. RESULTS AND REVIEW
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|Student Number |101 | | | | |Student Name |Sunil_3 Patel | | |
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base (NaOH). Salts formed from a strong acid and a weak base hydrolyze to form a solution that is slightly acidic. In this kind of hydrolysis‚ the water molecules actually react with the cation from the weak base. For example‚ when ammonium chloride‚ NH4Cl‚ hydrolyzes‚ water molecules react with the NH4+ ion: NH4+ + 2H2O ----------> NH4OH + H3O+ The formation of the H3O+ (hydronium) ion from this reaction makes the solution acidic. Salts formed from a weak acid and a strong
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(CaCO3). 1. CaCO3+2HCl-----CaCl2+CO2+H2O 2. CaCl2+K2CO3====CaCO3+2KCl The first reaction shows the separation of calcium carbonate from the mixture. In the second reaction we use the product of the first reaction (CaCl2) and change it back to calcium carbonate (CaCO3) by mixing CaCl2 with potassium chloride (2KCl). Objective To separate the components of mixture of sand‚ sodium chloride and calcium carbonate. Materials and Equipment 1. Two beakers 2. Experimental mixtures 3. Distilled water 4. Funnel 5
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Have you ever wondered why after finishing an ice cold drink on a hot day that the ice had altered itself into water? Water is actually made up of lots of tiny particles. These tiny particles move around in water when it is in its liquid form‚ but as the temperature gets lower these particles slow down and hardly move. When it gets cold enough they stick together and then what was once a liquid has now became a solid we all know as ice. Ice turns into water‚ back to a liquid‚ when the temperature
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Priestley is credited with the discovery of oxygen. He produced O.‚ by heating mercurv(II) oxide‚ HgO‚ to decompose it into its elements. How many moles of oxygen could Priestley have produced if he had decomposed 517.84 g of mercury oxide? 0. Iron(III) chloride‚ FeCl3‚ can be made by the reaction of iron with chlorine gas. How much iron‚ in grams‚ will be needed to completely react with 58.0 g of Cl2? 194. Sodium sulfide and cadmium nitrate undergo a double-displacement reaction as shown by the following
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any anion + hydrogen ion [H+ (aq)] = soluble hydrogen chloride‚ HCl‚ is soluble any anion + ammonium ion (NH4) = soluble ammonium chloride‚ NH4Cl‚ is soluble nitrate NO3- + any cation = soluble potassium nitrate‚ KNO3‚ is soluble acetate (CH3COO-) + any cation (except Ag) = soluble sodium acetate‚ CH3COONa‚ is soluble Chloride (Cl-)‚ Bromide (Br-)‚ Iodide (I-) + Ag+‚ Pb2+‚ Hg2+‚ Cu+‚ Tl+ = low solubility (insoluble) silver chloride‚ AgCl‚ forms a white precipitate + any other cation
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8/21/2009 |Secondary 2 | Shela Septania Usadi | [pic] Table of Contents Part 1: Abstract 1 Part 2: Introduction 1 Fire 1 Color Of Fire 2 Colored Flame 2 Part 3: A Simple Experiment‚ Green Flames 5 The Materials 5 The Method 5 A Higher Explanation 5 Part 4: Multicolored Fire 6 The Materials 6 The Method 6 Part 5: Uses Of Colored Fire 7 Part 6: Effects
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