titration of an acid and a base in order to determine the of the weak acid‚ . is a constant for a given acid at a given temperature. In this experiment we determined the Ka using two different methods: 1) the measurement of the pH of a solution containing a known concentration of a weak acid‚ and 2) measurement of the pH at the half-neutralization point in the titration of a weak acid and a strong base. Theory and Concept: When titrating a weak acid‚ HA‚ with a strong base the equilibrium between
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Observations of Chemical Changes Purpose/Hypothesis: To observe how acids react with bases and examine reactions of common household cleaners and the macroscopic changes these chemicals undergo. I expect for each solution to react differently when mixed with acids and bases. Procedure: I have a well-plate-96‚ a piece of white and black paper‚ and the chemicals from the Observation of Chemical Changes Experiment Bag. I used a different well for each combination of solutions. I placed two
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is the almost the initial volume of HCl. In Condition 2 Trial 2 the initial volume of HCl was 8.0 mL‚ the substance stayed pink at 16.0 mL‚ so the amount of NaOH needed for neutralization was 8.0 mL. In the other conditions and trials the most that base was off from the acid was 1 mL. The average HCl and NaOH stayed fairly close‚ this is shown in Fig 1. The Hypothesis was supported. Evaluation: Limitation/Design Error Specific Effect(s) on Data Way to fix it? The phenolphthalein dropper was
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delivery of 5 ml. of titrant b- at half-equivalence c-at equivalence d-after delivery of 23 ml. of titrant Part A) Reaction is: HNO2 + OH- NO2- + H2O Ka for Nitrous acid = 7.2E-4 Kw = Ka*Lb Kb = 1.0E-14/7.2E-4 Kb = 1.38E-11 Moles of base: (0.15)*(0.022) = 3.3E-3 moles 1:1 Ratio‚ So‚ Moles of acid = 3.3E-3 moles NaOH: (0.005)*(0.15) = 7.5E-4 moles HNO2: 3.3E-3 – 7.5E-4 = 2.55 E-3 moles Using Henderson- Hassel Balch equation: Ph = 4.752 + log(7.5E-4/2.55E-3) Ph =4.21 Part B) Ph = 4.752
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An acid-base titration is carried out by adding an acidic titrant to a basic solution. At which point should the titration be stopped and the volume of titrant used be recorded? Answer : when the solution reaches the endpoint Question = Buffers are substances‚ or mixtures of substances‚ that (help maintain a relatively constant pH when small amounts of acids or bases are added) Question= Which of the following statements best describes what determines whether an acid is a strong acid
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Purpose This experiment shows how different concentrations of acids and bases in a solution affect its pH level. When acids and bases are combined in a solution‚ they neutralize each other. This means that depending on the concentration of both acids and bases in a solution‚ the pH will vary. A neutral pH level is 7; anything below that level is known as an acidic solution‚ while anything above is known as a basic solution. To find out the pH‚ the solutions will be diluted and tested with different
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Importance of acids and base Acids and bases are very important to us because everything in our world is affected by them. We could not live in a world that is either too acidic or too base. Think about heart burn‚ to treat heart burn‚ we have to have an understanding of acids and bases. BASE 1. A base is any of various water-soluble compounds capable of turning litmus blue and reacting with an acid to form a salt and water. 2. A base is a substance that changes red litmus
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|pH from Lab |Acid or Base? |Solution Name (from Lab results) | |Solution 1 |6 |Base |Water | |Solution 2 |1 |Acid |Lemon Juice | |Solution 3 |12 |Base |Bleach
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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) H3C3H5O7 (aq) + 3 NaCl (aq)"
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Experiment 4 SOLUTION STOICHIOMETRY ACID-BASE TITRATIONS Determination of the Percent Acetic Acid in Vinegar Objectives: (1) To introduce and use the concept of solution stoichiometry (2) To specifically use solution stoichiometry to determine the percent of acetic acid in vinegar. (3) To prepare a standard solution by the method of titration. Consider the following balanced chemical equations: (1) HCl + NaOH ------> NaCl + HOH (2) H2SO4
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