concentration of HCl when titrated with a standardized NaOH solution‚ through means of the titration method. My hypothesis is When an unknown concentration of HCl is titrated with a known volume of standardized NaOH solution‚ one can gather enough data to determine the concentration of the unknown (HCl). My prediction is If an unknown concentration of HCl is titrated with a known volume of NaOH‚ then one can gather enough data to determine the concentration of the unknown which is HCl. Procedure Standardization
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nichrome wire Label REAGENTS 0.5 M CaCl2 0.5 M BaCl2 M NaOH 0.1 M AgNO3 0.5 M KCl 0.5 M KBr 0.5 M KI 2 M NH4OH M KCN % H2O2 2 M H2SO4 MnO2 Saturated FeSO4 0.1 M NaNO3 CH3COOH 0.5 M Na2SO3 0.1 M KSCN 2 N KOH 0.5 M K4[Fe(CN)6] 0.5 M FeSO4 0.5 M FeCl3 0.5 M Al2(SO4)3 2 N HCl 0.5 M LiCl 0.5 M NaCl 0.5 M KCl 0.5 M K2Cr2O7 96% H2SO4 III. EXPERIMENTAL PROCEDURE 1. Reactions of Cu2+ 10 drops of 2 M NaOH‚ 2 M NH4OH‚ 0.5 M K4[Fe(CN)6] was added in turn order into each
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__________________ MATERIALS AND PROCEDURE As per Essential Experiments for Chemistry pages 163–170 RESULTS TABLE 1 Equilibrium involving bromocresol green Initial colour of bromocresol green in water = Reagent added HCl (step 3) more HCl (step 4) NaOH (step 5) more NaOH (step 6) Stress Colour change and # of drops required Direction of shift ver. 02/2012 1 Chemistry 12 Unit 2 Reaction Equilibrium TABLE 2 Equilibrium involving iron(III) thiocyanate ion Colour of FeCl3
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Abstract By using acid-base titration‚ we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein’s color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of
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[pic] Drops |Water(HcL) |Water(NaOH) |Liver(HcL) |Liver(NaOH) |Egg White(HcL) |Egg White(NaOH0) |Potato(HCl) |Potato(NaOH) |Buffer(HCl) |Buffer(NaOH) | |0 |7 |4 |7.4 |5 |8.2 |7 |6.9 |4 |10.7 |10 | |5 |4.5 |7 |6.9 |6 |7.5 |8 |6.2 |5 |10.5 |10 | |10 |2.7 |9 |6.3 |6 |7 |9 |5.7 |5 |10.4 |11 | |15 |2.6 |12 |5.8 |6 |6.4 |9 |5.3 |6 |10.3 |12 | |20 |2.5 |12 |5.4 |6 |4.5 |10 |4.9 |7 |10.2 |12 | |25 |2.4 |13 |5.1 |6 |3.5 |10 |4.6 |8 |10.1 |13 | |30 |2.3 |13 |4.8 |6 |3.3 |11 |4.2 |8 |10 |13 | | 1.
Free PH Acid dissociation constant
5. Write a balanced reaction of zinc with HCl. 6. How many moles of HCl are needed to react completely with all of the zinc in a post 1982 penny? 7. In a procedure developed to determine the percent zinc in post 1982 pennies‚ 50 ml of an HCl solution was used to react (dissolve) all of the zinc in the penny. To ensure complete reaction‚ the solution contains twice as many moles of HCl that is actually needed. What concentration of HCl should be used? 8. In the scenario
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is noted for 4consecutive readings. 7. Dump out the water and return the copper cylinders to your lab instructor now. B. Measurements of H for neutralization reaction. 8. Add 50mL of distilled water to the cup‚ and pipet 10mL of standardized 3.0M HCL into the water in the cup.
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INTRODUCTION: Carboxylic acids are organic acids characterized by the presence of a carboxyl group‚ -COOH. This acid acts as a weak acid‚ which can react with a strong base. Carboxylic acids form hydrogen bonds with many water molecules and are more soluble with one to four carbon atoms. Also‚ it may have an R group that consist of hydrogen or an alkyl group that changes its water solubility. Carboxylic acids with low molecular weight have odor at room temperature and higher molecular weight
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Thymol Blue REAGENT ADDED STRESS (ION ADDED) COLOR OBSERVATION DIRECTION OF EQUILIBRIUM SHIFT HCl (Step 3) HCl (Step 4) NaOH (Step 5) NaOH (Step 6) Table 2 Equilibrium Involving Thiocyanatoiron (III) Ion REAGENT ADDED STRESS (ION ADDED) OBERSERVATION DIRECRTION OF EQUILIBRIUM SHIFT KCl (test tube B) Fe(NO3)3 (test tube C) KSCN (test tube D) NaOH (test tube E) Table 3 Equilibrium Involving Cobalt (II) Complexes STRESS OBSERVATION DIRECTION
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we use a strong acid (HCl) and a weak acid (acetic acid) titrates with a strong base (NaOH). In both titrations‚ we will monitor the change in PH to determine the volume of 0.100 M NaOH required neutralizing both 10ml sample of HCl and acetic acid. And refer to the neutralization reaction of these two acid‚ H+ (aq) + OH-(aq) → H2O(l) for HCl‚ and CH3COOH(aq) + OH-(aq) → CH3COO-(aq) + H2O(l) . as we can see ‚ in both case‚ two reaction have 1:1 stoichiometry‚ the moles of NaOH added = moles of acid
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