levels using a standard wide-range indicator. Based off of the results obtained in the lab room‚ fill in the following table: Solution Number pH from Lab Acid‚ Base or Neutral? Solution Name (what was in the test tube?) Solution 1 6 Neutral Water Solution 2 0 Acid Lemon Juice Solution 3 12 Base Bleach Solution 4 5 Base Coffee 1. How many drops of wide range indicator will you use for each test‚ based on industry standards such as the LaMotte field test? 1 drop Section 2: Now
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check the acidity and record result. Safety precaution: * Acid and base are corrosive‚ irritating to the skin and often release choking vapor. So avoid in contact with your skin‚ eye and skin protection should always be worn when using them. * Transfer by dropper only small amounts at a time. * Have alkali or acid on hand for neutralization in order to minimize the threat caused by accident spill of acid or base. * Neutralization
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during synthesis‚ and can’t go back together after the whole enzyme is completed. Our bases traveled the whole distance just like our neutral solution. Discussion & Conclusion: In this lab we learned that when catalase is mixed with an acid it denatures. The unexpected result was that I thought our base would denature also but instead it did not. My data doesn’t fully support my hypothesis because our base didn’t denature only our acids did. The next time we perform this experiment we should
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|4|~2.5| Questions 1. Compare and contrast acids and bases in terms of their H+ ion and OH- ion concentrations. Vinegar – Acidic with a low pH of around 3. Sodium – Basic – with a higher pH scale around 7.5 Milk – I thought would be basic but it’s actually more acidic‚ around 6.5 Orange Juice – Acidic actually around 3.5 Hand soap – Basic around 9 pH Lemon juice - most acidic thing I tested around 2.5 2. Name two acids and two bases you often use. Acids: I drink Orange Juce everyday along
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finished the substrate will have turned into products and these products detach itself from the enzyme. Denaturation is when proteins lose their tertiary or secondary structure by application of some external stress of compound‚ such as a strong acid or base‚ a concentrated inorganic salt‚ an organic solvent‚ or heat. (http://www.princeton.edu/~achaney/tmve/wiki100k/docs/Denaturation_(biochemistry).html) To denature is to slow down‚ speed up‚ or stop an enzyme from completing its process. Conditions that
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this lab the acid Potassium hydrogen phthalate and two unknown acids were titrated. We determined the molar mass of the Potassium hydrogen phthalate‚ for the unknown acids we calculated the molar mass and the Ka values. We used NaOH as the known base for titrating in all three of the titrations. Our ka value based on our titration curve of KHP was 6.9 (the equivalence point where the pH equals the pKa) and our unknown acids were determined to be Hexanoic Acid (with an actual molar mass of 116
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PRACTICAL 15: DETERMINATION OF HEAT OF NEUTRALIZATION Data collection: |Reaction |Initial Temperature/°C (±0.25) |Final Temperature of Mixture/°C (±0.25) | | |Acid |Base | | |HNO3 + NaOH |28.00 |28.25 |34.50 | |HNO3 + KOH |28.25 |28.25 |34.00
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Writing Practical Reports Aim: To observe what happens during and after a chemical reaction. Equipment: Concentrated nitric acid in a glass dropping bottle Small pieces of Copper 250ml Beaker 2 M Lead nitrate in a dropping bottle 2 M Potassium iodide in a dropping bottle 2 M Copper sulfate in a dropping bottle 2 M Sodium hydroxide in a dropping bottle 2 M Hydrochloric acid in a dropping bottle 4 Pyrex test tubes Test tube rack Spatula Bunsen burner‚ gauze
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it is also equally possible that the solution was not shaken properly in order to avoid the over-addition of sodium bicarbonate. The failure to perform these steps correctly could have resulted in this loss of product due to the fact that too much base could have reacted with the product‚ resulting in a product that could have been washed by water‚ but
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that an acid is a substance that donates hydrogen ions. Because of this‚ when an acid is dissolved in water‚ the balance between hydrogen ions and hydroxide ions is shifted. Now there are more hydrogen ions than hydroxide ions in the solution (2). A base can increase the pH level by providing hydroxide and then being removed. The buffer section of this lab was used to stabilize the level of pH using 4 different types of samples. The pH levels of the
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