apparatus Measurement Mass of eggshell = 3.15 ± 0.01 g Volume of HCl added = 50.00 ± 0.5 〖cm〗^3 Volume of solution = 250.0 ± 0.3 〖cm〗^3 Volume of NaOH pipetted = 25.00 ± 0.03 〖cm〗^3 Titration number Rough 1 2 Initial burette reading of NaOH/ ± 0.05 cm3 0.00 0.00 0.00 Final burette reading of NaOH / ± 0.05 cm3 11.80 11.70 11.20 Volume of NaOH titrated / ± 0.10 cm3 11.80 11.70 11.20 Titration table: data collected from burette of amount of HCl used for the colour of the solution with
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with a base that can neutralize it with less then the acidified lake water‚ I will also look for a base that can make sulfuric acid neutral As a class we got options to what we will conduct this experiment with the base I choose is Sodium hydroxide (NaOH) and for the indicator to show that this will make it neutral is the Universal Indictor I choose that indicator because it has a wide color spectrum when being neutralized. Predictions How much base do you think do you think it will take to neutralize
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FC024 10th Jun 2013 Monday 2-4 pm Scientific Principles and Enquiry (Working in Pairs) Experiment 1 – pH Titrations Introduction In quantitative chemical analysis‚ acid - base reactions are often used to provide a basis for various titration techniques. The equivalence points of acid - base titrations can be estimated from the colour change of chemical indicators‚ such as phenolphthalein‚ methyl red‚ methyl orange and so on. The choice of an indicator
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Experiment 2: Protein Hydrolysis and Characterization | Reagents | Principle | Test for | Positive Result | Negative Result | Biuret | CuSO4‚ NaOH | Complexation of Cu+2 with amide N atoms | Polypeptide bonds | Violet/purple solution | Blue color solution | Sakaguchi | 10% NaOH‚ 0.02% α-naphtol solution‚ 2% NaOBr | arginine condenses with α-naphtol and NaOH | Guanido group (arginine) | orange solution | light yellow solution | Ninhydrin | 0.1% ninhydrin solution (1‚2‚3-indanetrione monohydrate
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studied variables are air flow rate‚ foam height‚ initial sodium hydroxide concentration‚ surfactants and surfactant concentration. The experimental results indicate that the conversion in the reactor increases with the increase in air flow rate‚ initial NaOH conc. The nature of surfactant has considerable effect on the foamability of solution and its amount also alters the conversion of reactant. CONTENTS Sl. No. Topic Page No. 1 2 3 4 5 6 7 8 Introduction Literature Review Experimental Setup
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0981 |29.4 | Calculations were completed as follows: Vol. of NaOH added (mL) * 1L/1000mL * 0.981mol NaOH/L = moles of NaOH added For monoprotic acid (R-COOH): Moles of Acid = Moles of NaOH Mass of acid (g)/moles of Acid = Acid’s molar mass (g/mol) For Diprotic acid (R(COOH)2): Moles of acid = ½ * Moles of NaOH Mass of acid/moles of acid = Acid’s molar mass (g/mol) To further enforce the conclusions drawn regarding the acids identity
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Ammonia gas produced on warming. White ppt. [y] Soluble in excess aq. NaOH to form a colorless solution. [z] Zn2+ + 2OH- Zn(OH)2 (white ppt) Zn(OH)2 + 2OH- [Zn(OH)4]2- (aq) White ppt. [u] Ca2+ + 2OH- Ca(OH)2 (white ppt) Insoluble in excess aq. NaOH. [w] White ppt. [p] Soluble in excess aq. NaOH to form a colorless solution. [q] Al3+ + 3OH- Al(OH)3 (white ppt) Al(OH)3 + OH- [Al(OH)4]- (aq) White ppt. Soluble in excess aq. NaOH to form a colorless solution. Pb2+ + 2OH- Pb(OH)2 (white ppt) Pb(OH)2
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SSN COLLEGE OF ENGINEERING DEPARTMENT OF CHEMICAL ENGINEERING V Semester – CH 2307 TECHNICAL ANALYSIS LAB -2010 INDEX SHEET CYCLE ONE Date of Condn. Date of Subn. Sign 1 Estimation of COD of the given sample of water. 2 Estimation of Manganese in the given pyrolusite ore. 3 Estimation of Magnesium by EDTA method. 4 Estimation of purity of drug using pH meter. 5 Estimation of Ammonia in ammonium salts. 6 Polarimetric estimation of sugar
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0 mL of the dissolved borax was added to the cooled PVA solution in 1.0 mL aliquots. The cross-linking consisted of the addition of sulfuric acid and sodium hydroxide. 3.0 M H2SO4 was added to the mixture until it became faint red. 2.0 mL of 1.0 M NaOH was added to the mixture to neutralize the H2SO4. Originally‚ it was planned to measure viscosity quantitatively with a start and end position of the mixture. It was planned to time how long it takes for the ball bearing to move through the start and
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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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