Barium chloride Calcium chloride Copper (II) chloride Magnesium chloride Potassium chloride Sodium chloride Unknown solids containing a single cation and labelled X‚ Y and Z Apparatus: Bunsen burner Insulation mat Platinum wire (or Nichrome wire)‚ Watch glass Safety precaution: As concentrated hydrochloric acid is corrosive‚ skin contact should be avoided. It is preferable to use polythene gloves and wear goggles while handling it. Copper (II) chloride and barium chloride are highly
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answer. Mass/Mole Problems 1. Determine the molar masses of the following compounds: a. dinitrogen pentoxide c. sodium carbonate b. ammonium phosphate 2. Calculate the number of atoms in 20.0 grams of calcium. Road map: grams ( mols( atoms 20.0 g Ca x 1 mol Ca x 6.02 x 1023 atoms Ca 1 40.01 g Ca 1 mol Ca atoms 3. What is the mass of 6.20 moles of potassium
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and include sodium‚ potassium‚ chloride‚ calcium‚ phosphorus and sulfur. Microminerals or trace elements are needed in smaller quantities and include iron‚ copper‚ zinc‚ selenium and iodine amongst others. Although trace elements are needed in smaller amounts‚ they are just as essential to health as major minerals. Minerals are essential to various functions in the body. Sodium‚ potassium and chloride are all necessary for fluid balance. Magnesium‚ sodium‚ calcium and potassium are critical for
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taking notes of what we observed. The different salts included Potassium chloride‚ Calcium chloride‚ Strontium chloride‚ Lithium chloride‚ Copper II chloride‚ Sodium Chloride‚ and Barium Chloride. Burning a pinch of each salt separately by holding a nichrome wire over a Bunsen burner‚ we found that each salt emitted a different color of light. For example‚ Potassium Chloride burnt a bright pink flame when burned‚ while Calcium burnt orange. No color was truly identical. What was the cause of this phenomenon
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Title : Osmosis in Quail’s Eggs Research Question What is the effect of different concentrations of sodium Chloride (NaCl) on the mass of the de-shelled quail’s eggs? Introduction Osmosis is an example of passive transport. Osmosis is defined as the movement of water molecules‚ down its concentration gradient‚ from an area of high water concentration (low solute concentration) to an area of lower water concentration (high solute concentration) through a selectively permeable membrane. Osmosis
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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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pipets (2) | |conductivity tester |CaCl2 (calcium chloride) | |ethanol |KI (potassium iodide) | |iron ring |NaCl (sodium chloride) | |ring stand |C13H18O2 (ibuprofen)
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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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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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