Analysis of the nitrogen content of lawn fertiliser 1. Aim To find the percentage by mass of available nitrogen‚ present as the ammonium ion‚ in a lawn fertiliser. 2. Materials 1.3g lawn fertiliser‚ finely ground 100ml standard sodium hydroxide solution (0.96M) 100ml standard hydrochloric acid (0.94M) Methyl red indicator 500mL de-ionised water Wash bottle containing de-ionised water Red litmus paper 2 × small funnels 250 mL volumetric flask 3 × 250mL conical flask 20mL pipette
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Solutions Chem 1290-016 03-05-2010 ------------------------------------------------- Purpose: The purpose of this lab was to use acid-base titrations to find the mass percent of ascorbic acid in a Vitamin C tablet. A known concentration of sodium hydroxide was used and the value found was compared to the stated amount of ascorbic acid listed on the vitamin container. Also in this lab the acidity of different salt solutions were tested using different indicators including litmus paper. Procedure:
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This experiment aims to discover the effect of 6 different treatments on the permeability of the cell membrane. These will be distilled water‚ sucrose‚ sodium hydroxide‚ hydrochloric acid‚ ethanol and boiled water. The treatments include immersion in these solutions‚ and exposure to high temperature. The tissue used is from the taproot of a beetroot‚ and the effect on the membrane’s permeability assessed by the amount of pigment leakage that occurs. Hypothesis ==========
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water as well as the density was calculated. The same process was performed to calculate the density of an unknown substance. The third part Section C 5-25% of sodium chloride was prepared by the instructor. For each percent concentration of sodium chloride a 25 mL was prepared. Weighing the graduated cylinder before and after the sodium chloride was transferred the density were calculation. Pre- Laboratory Questions: 1. A metal sphere weighing 15.45 g is added to 21.27 mL of water in a graduated
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to get the most accurate amount of base‚ to neutralise the acid. 1.2 Aim To determine the concentration of acetic acid in some commercial vinegars by titration against a standard sodium hydroxide solution. 1.3 Hypotheses It is hypothesised that as the volume of vinegar is increased‚ the amount of sodium Hydroxide required will neutralise will the acid to change it to a pale pink. Method 2.1 Materials * Diluted vinegar solutions (labeled ‘A’‚ ‘B’‚ & ‘C’) * Standardized 0.1M NaOH
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FREE FATTY ACID TEST AIM: To determine seed FFA MATERIALS REQUIRED Chemcals required * Oxalic acid pellets * Sodium hydroxide pellets * Rectified spirit * Phenolphthalein * Distilled water Apparatus required * 250ml standard flask(oxalic acid) * 1l std flask(sodium hydroxide solution) * 50ml beaker for solution preparation * 250ml beaker for solution preparation * Spatula * 50ml burette with standard for titration * 100ml conical
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manner. Solutions of sodium hydroxide are commonly used in titration analysis of samples containing an acidic solute. Although sodium hydroxide is a solid‚ it is not possible to prepare standard sodium hydroxide solutions by mass. Solid sodium hydroxide is usually of questionable purity. Sodium hydroxide reacts with carbon dioxide from the atmosphere and is also capable of reacting with the glass of the container in which it is provided. For there reasons‚ sodium hydroxide solutions are generally
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| What is observed | 1. Started with copper‚ Cu (s). | reddish‚ brownish‚ orange-ish‚ powder-like | 2. Added nitric acid‚ HNO3 (aq). | acid turns blue and smells like chlorine. | 3. Added water‚ H2O (l). | stayed the same | 4. Added sodium hydroxide‚ NaOH (aq). | changed consistency‚ gel-like | 5. Heated the mixture | becomes darker‚ dark-brown-like‚ shavings | 6. Filtered the solid and added sulfuric acid‚ H2SO4 (aq)‚ to it. | sulfuric acid cleans off the copper | 7. Added zinc
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use this experience to experimentally determine the concentration of acetic acid in an unknown solution. There are three parts to this experiment‚ they are 1. Preparation a standard solution of oxalic acid (~0.07 M) 2. Preparation a sodium hydroxide solution (~0.1M) which will be standardized using the standard oxalic acid solution. 3. Determination of the concentration of acetic acid in an unknown vinegar solution. (0.1-0.2M) Introduction Standard solutions are solutions with
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the cation of the base mixes with the anion from the acid‚ forming a base‚ and the hydrogen from the acid mixes with the anion from the base‚ forming water. In this reaction‚ the sodium ion from the sodium hydroxide attracts to the acetate ion from the acetic acid‚ and the extra hydride ion bonds with the negative hydroxide ion to form water. The water produced by the reaction had a pH of seven‚ and so when the whole solution was light pink‚ we knew the reaction had fully
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