be dropped into the flask for the endpoint to be visibly reached. This process would be repeated multiple times to eliminate random error. (Svante) In this lab the base NaOH will be used to fill the buret and act as the titrant. Then flasks of acetic acid solution will be placed beneath the buret full of NaOH. Then‚ the base will slowly be added to the solution until the endpoint is reached and the bright pink color fills the liquid inside the container. Once the reaction has reached completion
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Abstract For the amount of aspirin in a commercial tablet to be determined‚ different solutions of acetylsalicylic acid mixed with NaOH were created at different concentrations. All the different solutions were then analysed using Novaspec photometer‚ which allowed for a graph to be created and a line of best fit to be made. The amount of aspirin in a commercial tablet was found to be 350mg. Introduction The molecular formula for aspirin‚ also known as acetylsalicylic acid‚ is C9H8O4. It is most
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aqueous hydroxide ion (OH-). CatOH ( Cat+ + OH- K (Kb since it is a base) is large‚ but since the equilibrium is for a base‚ we use the value pKb to describe the degree of dissociation. Ka x Kb = Kw Ex: sodium hydroxide‚ NaOH What is the pH of a 0.003 M solution of NaOH? NaOH ( Na+ + OH- [OH-] = 0.003 M pOH = 2.52 pH = 14 – pOH = 11.48 (basic) Weak acid: If the acid does not dissociate completely in H2O‚ then it is a weak acid. (note: H2O does not dissociate completely‚ so it is a weak
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r Lab Report 5 Introduction to the Classes of Chemical Reactions Course: Chem. 1151L‚ Tuesday & Thursday June 23‚ 2011 Mr. Nasir Uddin Pre Lab Questions: 1. CaBr2 (aq) + K3PO4 (aq) → CA(PO4)2(S) + KBr (aq) = Ca3(PO4)2 + 6 KBr Double Replacement 2. Li(s) + O2(g) = Li2O(s) =2 Li2O Decomposition 3. CH4 + O2 = CO2 + H2O = CO2 + 2 H2O Combination 4. AgBr(s) = Ag (s) + Br2(l) = 2 Ag + Br2 Combination 5. Mg(s) + H2SO4 (aq) = MgSO4 + H2
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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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heat of neutralization for the reaction of sodium hydroxide (NaOH) and hydrochloric acid (HCI). Requirement The heat of neutralization (∆Hneutzn ) is the heat transferred when 1 mol of an acid reacts with 1 mol of a base. This heat is generally reported in either kilojoules per mole (kJ/mol) or kilocalories per mole (kcal mol). The reaction of HCI and NaOH solutions is shown in Equation 1. HCI(aq) + NaOH(aq) H20(l) + NaCI(aq) (Eq
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Hydrochloric Acid in a Given Solution by ARAKA BRAMWEL MBOGO EN251-0221/2010 TITLE: STANDARDIZATION and DETERMINATION OF THE CONCENTRATION OF HYDROCHLORIC ACID PRESENT IN A GIVEN SOLUTION Aims: To be able to standardize Sodium Hydroxide (NaOH) solution using a standard solution of Oxalic acid. To be able to prepare standard solutions. To determine the strength of a given solution of Hydrochloric acid (HCl) To analyze errors that occur during standardization experiments. Introduction:
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Tittle : Rancidity Measurement in Fats and Oils. Introduction : Vegetable oil is an important and widely used lipid source for our everyday food products. Its application is increasing day by day for food purposes and for the manufacturing of a number of toiletry products. However‚ some vegetable oils are not up to standards to meet consumer satisfaction in terms of their physico-chemical properties or for the texture and stability of the food products (Reyes- Hernandez et al.‚ 2007). Recently
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series of steps‚ the sum of the enthalpies for each step equals the enthalpy change for the overall reaction. For example‚ the three chemical equations used throughout the experiment were: Equation 1: NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) Equation 2: NH4Cl(aq) + NaOH(aq) NH3(aq) +NaCl(aq) + H2O(l) Equation 3: NH3(aq) + HCl(aq) NH4Cl(aq) Resulting in Equation 1 plus Equation 2(reversed) will equal Equation 3. In this case‚ Hess’s Law gave the ΔH for Equation 3. Calorimetry is the
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Test Biuret Test Reagents CuSO4 sol’n‚ diluted NaOH Test for Intact proteins and protein hydrlysates (at least tripeptide‚ 2 peptide bonds Result Pink to violet blue color Ninhyrin Test 1‚2‚3-indanetrione monohydrate or triketohydintene hydrate‚ ethanol Alpha- amino group (usually a general test for amino acids) Xanthoproteic Test Conc. HNO3‚ conc. NaOH For W‚F‚Y (aromatic except for H) Blue to blue-violet Oxidative decarboxylation color & deamination
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