amounts of strong acids or base are added to it. (Boundless‚ 2015) This is usually formed when a weak acid is added to a salt of its conjugate base. (Chemicool.com‚ 2014) When an Alka Seltzer tablet is dissolved in water‚ a buffer is formed when the weak acid citric acid is present with sodium citrate (citrate ion) the conjugate base (Buffer Balancing Acts Buffers‚ 2009) "Na3C3H5O7 (aq) + 3 HCl (aq) H3C3H5O7 (aq) + 3 NaCl (aq)" (Senese‚ 2010) By exchanging the Na+ in sodium hydrogen carbonate
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Rates of Reaction Coursework Aim: To find out how different concentrations of sodium thiosulphate (Na S2 O3) affects the speed of its reaction with Hydrochloric acid (HCL). Introduction When Sodium Thiosulphate and Hydrochloric acid react they produce a cloudy precipitate. Both of the chemicals are clear solutions and they react together to form a yellow precipitate of sulphur‚ the equation for this reaction is: Na2 S2 O3 + HCL‚ H2 O + NaCL + SO2 + S Sodium Thiosulphate + Hydrochloric
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volumes form my results table which I have added them and then divided by three to get an average results. Describe the stages you followed in collecting the primary data and any secondary data. Titration Steps: • Firstly we weighed the solid sample of sodium hydrogen carbonate with an accurate balance; then dissolved in distilled water up to 250ml to make a
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Some metals react with acids while others do not. In this experiment‚ students will perform 2 reactions: aluminum/zinc with excess 6M hydrochloric acid and aluminum-zinc alloy with excess 6M hydrochloric acid. The purpose of this experiment is to determine the atomic mass of each metal and the percent composition of a known mass aluminum-zinc alloy by determining the moles of H2 gas formed. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) 1 mole of H2(g) is produced for every 1 mole of Zn(s) 2. 2Al(s)
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Zinc and Hydrochloric-Acid Written By Kahlil Zione Date:02/02/05 Abstract: We observed the reaction between zinc and hydrochloric acid and recorded it in a table and learned wether the percentage of zinc is effected by the amounts of both substances added to the solution. Introduction The purpose of this experiment is to determine if the amount of zinc and hydrochloric acid will effect the percentage of the zinc in the out coming solution. We are reacting zinc metal with hydrochloric
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Carbonates react with strong acids to give off carbon dioxide and water. Marble is calcium carbonate and thus behaves in the same way: CaCO3 (s) + 2HCL (aq)  CaCL2 (aq) + H2O (l) +CO2 (g) In this experiment‚ I am going to see if temperature affects the reaction rate between marble chips and hydrochloric acid by timing the release of carbon dioxide in the reaction. I predict the higher the temperature‚ the faster the reaction rate. This is due to the kinetic theory. The more heat
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Finding the Activation Energy of the reaction between Hydrochloric Acid and Sodium Thiosulfate The equation for the reaction is: S2O32- (aq) + 2H+(aq) ⋄ SO2 (g) + S(s) + H2O (l) Equipment - 2 boiling tubes - 400 cm3 beakers - Marker pen - Stand and clamp - Timer - Bunsen burner‚ tripod and gauze - 0 – 100 oC thermometer - 2 x 10 cm3 measuring cylinders - Access to a fume cupboard. Method 1. Label two boiling tubes A and B. Mark a dark spot on the side of a 400cm3 beaker‚ then ½ fill
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between the two metals in the metal sulfate solution of the electrolyte. In order for a chemical reaction to take place‚ the reactants must collide. The collision between the molecules in a chemical reaction provides the kinetic energy needed to break the necessary bonds so that new bonds can be formed. Thus‚ increasing the concentration of the anode‚ zinc sulfate‚ will increases the rate of reaction for oxidation because there are more zinc ions in the new concentration‚ which would also increase
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Publication No. 91860 Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid Rate Laws Introduction The purpose of this demonstration is to investigate the effect of sodium thiosulfate concentration on the rate of reaction of sodium thiosulfate with hydrochloric acid. The reaction‚ which produces solid sulfur‚ will be followed by measuring the time needed for the reaction mixture to become opaque. The results will be analyzed graphically to determine the order of reaction— the mathematical relationship
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E XPE RIME NT 4 . 5 Reactions of acids Aim To investigate and compare some reactions of a strong acid‚ hydrochloric acid‚ and a weak acid‚ ethanoic acid (common name‚ acetic acid) Equipment Dropper bottles containing: • 0.1 M hydrochloric acid‚ HCl • 0.1 M ethanoic acid (acetic acid)‚ CH3COOH • 0.1 M sodium hydroxide‚ NaOH • 1 M hydrochloric acid‚ HCl • 1 M ethanoic acid (acetic acid)‚ CH3COOH • universal indicator solution • limewater (calcium hydroxide‚ Ca(OH)2) Marble chips (calcium carbonate
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