Acetate formula | CH3COO- | 5 | Ammonia formula | NH3 | 6 | Nitric acid formula | HNO3 | 7 | Phosphoric acid formula | H3PO4 | 8 | Sodium phosphate formula | Na3PO4 | 9 | Calcium carbonate formula | CaCO3 | 10 | Ammonium sulfate formula | (NH4)2SO4 | 11 | Carbonic acid formula | H2CO3 | 12 | Sodium bicarbonate formula | NaHCO3 | 13 | Sodium hydroxide formula | NaOH | 14 | Calcium hydroxide formula | Ca(OH)2 | 15 | Ethanol formula | C2H5OH | 16 | Hydrobromic acid formula |
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two drops from chemical 1 and two drops of chemical two‚ unless otherwise stated‚ then recording the type of physical reaction or color changes that occurred. Well#/questions Chemicals Reactions A NaHCO 3 and HCI - C0 2 When combined Sodium Bicarbonate and Hydrochloric Acid‚ Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced. B HCI and BTB When Hydrochloric acid and Bromothymal blue are combined there is a physical change
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Purpose: The purpose of the practical that we completed was to determine the molar mass of carbon dioxide (CO2) by experimental means and to observe the reaction of hydrochloric acid and sodium carbonate. Using the balanced equation: Na2CO3 + 2HCl → 2NaCl + H2O + CO2 Materials / Apparatus: 1) 8.00g of sodium carbonate‚ 2) 30mL of hydrochloric acid (6molL-1) 3) 100mL of hydrochloric acid (6molL-1) 4) 100mL conical flask‚ 5) 150mL glass beaker 6) 50mL glass beaker 7) Glass funnel‚ 8) Digital scales
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ammonium ions (NH4+) are called ammonium salts. NOTE: •An anion is a negatively charged ion. Hence:•Hydrochloric acid gives chlorides. E.g. sodium chloride‚ ammonium chloride. •Nitric acid gives nitrates. E.g. barium nitrate‚ copper nitrate. •Sulphuric acid gives sulphates. E.g. silver sulphate‚ iron (ii) sulphate. •Phosphoric acid gives phosphates. E.g. sodium phosphate‚ ammonium phosphate. •Each acid gives rise to a series of salts named by the ANION which they contain. •Some acids can donate more
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Name: Kamaal Thomas |Date: January 4‚ 2011 | |Graded Assignment Lab Report Answer the questions below. When you have finished‚ submit this assignment to your teacher by the due date for full credit. (8 points) |Score | | | 1. For Part 2: Single-Displacement Reactions: For each of the four single-displacement reactions‚ describe what happened in each well. If a chemical reaction occurred‚ write a balanced equation for it. Then using the A‚ B symbols‚
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It is clear that salt‚ also known as sodium chloride‚ should no longer be used on our roads in the winter months. The first two reasons why salt needs to stop being used are because salt negatively affects aquatic ecosystems and causes damage to vegetation. The third reason is because thankfully‚ there are alternatives that we can use‚ that would be benefiting us which we should use instead of sodium chloride. To begin with‚ sodium chloride is detrimental to our aquatic ecosystems when it is
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aqueous solutions of calcium chloride and sodium carbonate. These solutions will be prepared from 2.01 g of calcium chloride and 1.06 g of sodium carbonate . Materials: 3 beakers 100 mL graduated cylinder rubber policeman funnel filter paper Procedure: 1. Put on your safety goggles. 2. Obtain two clean beakers. Rinse the inside of the beakers with a small amount of distilled water. 3. Obtain the correct amounts of calcium chloride and sodium carbonate. Enter these masses in your
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Experiment 11 Date: 28-3-2011 Title: Interpretation of reaction by the Le Chatelier’s principle Objective: To determine the factors that affecting the equilibrium position Introduction: Le Chatelier’s principle states that if a system in equilibrium is subjected to a change‚ the equilibrium position of the system will shift in a direction to minimize the effect of the change. Iron(III) ions and thiocyanate ions (NCS-) react in solution to produce thiocyanatoiron(III) (FeNCS2+)‚ a
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Investigating Chemical Equilibrium (Experiment 19 A) Purpose: 1. to recognize the macroscopic properties of five chemical systems at equilibrium 2. to observe shifts in equilibrium concentrations as stresses are applied to the systems 3. to observe a shift in equilibrium concentrations associated with changes in temperature 4. to explain the observations obtained by applying Le Chatelier’s principle Materials Required: See page 209 Heath Chemistry Laboratory Experiments Procedure:
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Data 1. Record your data for each of the trials in Table 2. 2. Record your reaction observations (Step 8) below: A white powdery substance formed when the two reactants were mixed Table 2: Reaction product data Mass (g) Example Trial 1 Trial 2 Mass of CaCl2 1.00 2.00 3.00 Mass of K2CO3 2.5 g 2.50 2.50 Mass of filter paper 0.8 g 0.80 0.80 Mass of watch glass 38.5 g 38.5 38.5 Combined mass of product‚ filter paper‚ and watch glass 40.2 g 42.3 43.3 Mass of dry product 0.9 g 2.00 3.00 Calculations
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