- 8.2 Bleach - 12 - 12.0 Ammonia - 12 - 11.0 Questions 1. Compare and contrast acids and bases in terms of their H+ ion and OH-ion concentrations. When an acid is dissolved in water‚ there are more hydrogen ions(H+) present than hydroxyl ions(OH-) due to the fact that acids donate hydrogen ions. An alkaline or basic solution accepts hydrogen
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Standardization of Solution and Titration Lab Report‚ Preparing a Dilute HCl Solution from a Concentrated One Titrating NAOH Solution with HCl Solution (of Known Concentration) Chemistry lab report(by abdazino abdalla) International College Objective preparing a dilute HCl solution from a concentrated one titrating NAOH solution with HCl solution (of known concentration) Procedure Section A: Preparation of 100.0cm3 0.480 mol/dm3 HCl solution a)Determine the volume of the concentrated acid
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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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determine the concentration of an acid or base in a solution. This process involves a solution of known concentration delivered from a buret into the unknown solution until the substance being analyzed is just consumed. In this lab‚ experimenters using hydrochloric solution to react with the solution of NaOH according to this equation: HCl (aq)+ NaOH(aq) → NaCl(aq) + H2O(l) HCl is a strong acid‚ NaOH is also a strong base‚ therefore they will dissolve completely
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underneath the well plate B. HCl + BTB C1 Once I added the Bromothymol Blue indicator‚ it turned an orange-like color C. NH3 + BTB E1 The reaction turned dark blue. When Bromothymol Blue reacts with an acid‚ it turned orange‚ and when it reacts with a base‚ the end result is blue. D. HCl + blue dye G1 The reaction turned green. E. Blue dye + NaOCl A3 The reaction turned blue. with the 1 drop of HCl A3 The reaction turned from blue to a blotchy bowl of blue‚ green‚ and yellow. Similar to oil
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for pH 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 7 Neutral Pure Water Solution 2 1 Acid Lemon Juice Solution 3 12 Base Bleach Solution 4 5 Acid 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? For
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take a small amount of the material you are using and hold it up to a flame and it turns a yellow/pinkish blue color‚ you also might have sodium bicarbonate. B. You know what color phenolphthalein and bromothymol blue turn when testing an acid or a base. Use the empty pipet in the Auxiliary Supplies Bag to test several (at least 3) household items including household cleaning products with bromothymol blue. Rinse the pipet well before using it on the next household chemical. When finished with this
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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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Observations of Chemical Changes Experiment 1 Chemistry 111 September 3‚2014 Ashley Mattox Abstract: The purposes of this lab is to observe the reactions of some common chemicals contained in consumer products and observe the macroscopic changes these chemicals undergo. Purpose: The purpose of the lab is to be able to interpret underlying macroscopic changes in terms of the behavior of atoms and molecules and also to learn how to separate mixtures into their component
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react when the equilibrium has been distressed. Objective: You will observe the application of Le Chatelier’s principle by observing the effects of acids and bases of on the solubility of Ca (OH) 2‚ the effects on Fe3+ and SCN- with Fe (SCN) 2+ to an equilibrium mixture. Also‚ finding the effects of an acid and base dealing with an indicator‚ and the effect on an acid on Ni2+‚ NH3‚ and Ni (NH3)62+. Data and Data Analysis: • Ca(OH)2 [pic] Ca2+ + 2 OH-
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