1.1.1 Galacturonic Acid Analysis (for Pectin Analysis) Defattening of Mango Peel Powder (Tunchaiyaphum et al.‚ 2013) 1. Weigh about 3 g sample and put into thimble of the soxhlet extractor. 2. Pour in 150 mL of absolute ethanol to the flask of the soxhlet extractor. 3. Extract at boiling temperature of ethanol for 4 hours. 4. Remove solid contents from the thimble. Set aside to dry. Acid Hydrolysis of MPP (Rehman et al.‚ 2004) 1. Mix defatted peel powder with water at pH 2.5 adjusted w/ 0.1 N H2SO4
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reacts with dilute acids. Planning What I am going to do I am going to find out how much heat is given out when magnesium reacts with a variety of dilute acids. In order to make comparisons between the acids‚ I shall use my results to work out how much heat would be given out if 1 mole of magnesium reacted with an excess of each acid. The acids I shall use are hydrochloric acid‚ sulphuric acid‚ nitric acid and ethanoic acid. What I already know Magnesium reacts with most dilute acids to give a magnesium
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Any strong acid will release approximately - 57 kJ/mol of energy on neutralisation with strong base. This energy release is due to the formation of water molecules from the H+ ions from the acid reacting with the OH- ions from the base. H+(aq) + OH-(aq) H2O(l) When a weak acid is neutralised some of the energy is needed to dissociate the molecules to make the hydrogen ions available for neutralisation. The result is a value for neutralisation enthalpy lower than - 57 kJ/mol (numerically
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__________________________________________________________ INTRODUCTION Monitoring the pH range of a laboratory reaction or a process is very important. It is important to keep the pH almost constant even when addition of acids or bases takes place. One can easily know if a solution is an acid or a base using a visual indicator. Indicators are organic dye added to a solution that changes color base on the concentration of H3O ions in the solution. Each color change corresponds into a pH value
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solution is known as a homogeneous mixture of two or more substances. For example‚ vinegar is a solution of acetic acid‚ the solute‚ in water‚ the solvent. A buffer solution is one which resists changes in pH when small quantities of an acid or an alkali are added to it. An acidic buffer solution is simply one which has a pH less than 7. Acidic buffer solutions are commonly made from a weak acid and one of its salts often sodium salt. An alkaline buffer solution has a pH greater than 7. Alkaline buffer
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using a premade cabbage juice indicator. Introduction Acids and bases are chemicals commonly used in the lab‚ and‚ even though we may not realize it‚ they are also found in substances we use at home on a daily basis. To test the acidity or basicity of a substance‚ we can titrate each until the endpoint is reached‚ or use an indicator. Something as simple as litmus paper can be used‚ whereby blue litmus paper will turn red in the presence of an acid‚ and bases will turn red litmus blue. We can also use
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Aim: To verify the buffering capacity of a phosphate solution using a pH meter and construct a titration curve of an amino acid to determine the pka values of its ionisable groups to identitfy an unknown amino acid. Method: The ratio of [HPO42-] to [H2PO4-] required to produce buffer solutions at pH values 5.9‚ 6.9 and 7.9 were calculated. 0.1M of H2PO4- and 0.1M HPO42- were used to mix appropriate volumes to 25mL of each of the buffer solutions. The calibrated pH meter was used to measure
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amount of various metals and minerals. When these metals come in contact with acid rain there can be some harmful chemical reactions. These reactions can lead to soil erosion. Acid rains are known to reduce the fertility of the soil‚ leaving the land barren. Harmful acids can also reduce the amount of soil micro organisms which perform important job of breaking down the dead and decayed plants and other beings. Rainfall: Acid soils are most often found in areas of high rainfall. Excess rainfall leaches
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Phenol‚ also known as carbolic acid‚ is an aromatic organic compound with the molecular formula C6H5OH. It is a white crystalline solid that is volatile. The molecule consists of a phenyl group (-C6H5) bonded to a hydroxyl group (-OH). It is mildly acidic‚ but requires careful handling due to its propensity to cause chemical burns. Phenol was first extracted from coal tar‚ but today is produced on a large scale (about 7 billion kg/year) from petroleum. It is an important industrial commodity as a
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ANSWERS TO QUESTIONS: 1. a. in distilled water: Cu(OH)2(s) (( Cu2+(aq) + 2OH-(aq) Ksp Cu(OH)2 Keq = Ksp Cu(OH)2 = 2.2 x 10-20 b. + 6.0M H2C2O4 Cu(OH)2(s) (( Cu2+(aq) + 2OH-(aq) Ksp Cu(OH)2 H2C2O4 (( H+ + HC2O4- Ka1 H2C2O4 HC2O4- (( H+ + C2O42- Ka2 H2C2O4 Cu2+ + C2O42- (( CuC2O4 1/Ksp CuC2O4 2(OH- + H+ (( H2O) 1/K2w Net Keq = (Ksp Cu(OH)2 x Ka1 x Ka2 )/Ksp CuC2O4
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