ICSE Class X Chapter 5 Hydrogen Chloride and Hydrochloric Acid Hydrogen chloride (HCl) : Formula : HCl Nature : Covalent. Molecular Mass : 36·5u [i.e. HCl = 1 + 35·5 = 36·5] Occurrence : (i) Present in gastric juices. (ii) Present in volcanic gases. Laboratory preparation of HCl gas : Hydrogen chloride gas is prepared in laboratory by heating conc. H2SO4 with NaCl. NaCl + H2SO4 Heat → NaCl + NaHSO4 Heat → NaHSO4 + HCl Sodium hydrogen sulphate Na2SO4 + HCl
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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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A buffer is an aqueous solution that allows resistance to significant change in pH when small 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)
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it will show a colour change. After that record the initial reading of the burette and making sure that all your burette readings must be to an appropriate precision. Titrate the contents of the conical flask by adding to it 0.100 mole dm3 hydrochloric acid from the burette. Add the solution slowly. Swire the flask gently to mix the contents at the end indicator turns as define red colour. This is the end point of the titration. Record the final burette reading in your table of result. Repeat the
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the hydrochloric acid to produce hydrogen gas. This is because magnesium is higher than hydrogen in the reactivity series. Therefore‚ when the two reactants are combined‚ a displacement reaction occus and the magnesium displaces the hydrogen‚ forming magnesium chloride and hydrogen gas. Mg (s) + 2HCl (aq) -> MgCl 2 (aq) + H 2 (g) Magnesium + Hydrochloric acid -> Magnesium Chloride + Hydrogen Aim The aim of this investigation is to observe the effect that
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Acid in the human stomach When people refer to acid they usually see it as a corrosive liquid that can dissolve metals or change the color of a substance. So they think of acid as a dangerous matter for the body and believe it can easily dissolve your skin. What I have previously listed are indeed properties of certain acids‚ such as Hydrofluoric Acid which can cause irreversible tissue damage if it comes in contact with skin‚ but not all acids are this strong. As a matter of fact what a lot of
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investigation into the effect of changing the concentration on the rate of reaction Aim: To investigate into the effect of changing the concentration on the rate of reaction Variables: · Keep the same volume · Keep the same length of magnesium · Change the amount of acid · Change the amount of water Method: · Set up apparatus as shown · Add 30ml of hydrochloric acid into the beaker · Measure 5cm of magnesium · Add the 5cm of magnesium to the hydrochloric acid · Put a bong onto the
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Sodium thiosulfate is safe to handle and store‚ but if it is mixed with an acid‚ a reaction happens. When dilute sodium thiosulfate is mixed with an acid‚ solid sulphur is made‚ which makes the solution appear cloudy. The reaction also makes small amounts of toxic sulphur dioxide gas. You will choose one factor and investigate this factor’s effect on the rate of reaction between sodium thiosulfate and dilute hydrochloric acid. A colorimeter is a device used in colorimetry that generally refers to
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STANDARDISATION OF HYDROCHLORIC ACID REPORT Aim: To standardize an unknown solution of hydrochloric acid Method: See INSTRUCTIONS for practical 6.2 & 6.3 Results: Attempt No. | Titre (mL) | | 1 | 20.9 | Rough Titration | 2 | 20.5 | | 3 | 20.7 | Concordant Titres | 4 | 20.7 | | 5 | 20.7 | | (1) Tabled Results (2) Concordant Titrations Results 20.7 mL | 20.7 mL | 20.7 mL | Average of Concordant: (20.7 + 20.7 +20.7) 3= 20.7 mL Calculations:
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(Fe3+ ) form. Ferric form is not usually absorbed in the body. In the stomach‚ there is low pH of 2 due to presence of gastric acids such as Hydrochloric and Ascorbic acids. These acids provide an acidic environment for reduction of ferric iron to ferrous (Fe2+). Ferrous iron can be absorbed in the body system. As in following equation of iron (iii) reaction with Ascorbic acid ‚ the product is iron (ii) chloride which is soluble 2 Fe3+ (s) + C6 H8 O6 (aq) → 2 Fe2+ (aq) + C6 H6 O6 (aq) + 2 H (aq)+
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