Abstract Titration is a laboratory method in which the endpoint of a reaction is determined quantitatively. In this experiment‚ the amount of soda ash present in a sample was determined and the alkalinity reported as it was titrated using HCl as the titrant. Also‚ the percentage amount of Na2CO3 and NaHCO3 present in the sample was determined at the end of the experiment. Introduction Soda Ash (Na2CO3) or sodium carbonate is commonly used as a cleaning agent and known as “washing
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1034 ppm‚ with a standard deviation of 2.4495. The results indicate that the unknown solution can be considered as hard water. Introduction The hardness of water is defined in terms of its cation content‚ which includes calcium‚ magnesium‚ iron‚ zinc‚ and other polyvalent metal ions. These metal ions interfere with the use of the water for many applications. For example‚ these ions diminish the effectiveness of soap and detergent for cleansing operations; they diminish the drinking quality of
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Reshmi Nair Title: Determination of Aspirin through back titration. Aim: To determine the concentration of Aspirin in a tablet using NaOH and Hcl. Research Question: What is the concentration of Aspirin in a normal tablet? Background: Aspirin is the general name for acetylsalicylic acid (ASA); it is also the trademark of the drug produced by Bayer in Germany. In eighty countries‚ aspirin is a registered trademark‚ but in other places the term aspirin refers to ASA by itself or as an ingredient
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provided pre-diluted chemicals. Utilizing the 96-well plate‚ 2 pipit drops of each chemical were added to the wells in the following combinations: a) NaHCO3+HCl b) HCl+Bromthymol blue c) NH3+1 drop Bromthymol blue d) HCl+blue dye e) Blue dye+NaOCl followed by HCl f) NaOCl+KI followed by various test foods g) KI+Pb(NO3)2 h) NaOH+phenolphthalein i) HCl + phenolphthalein j) NaOH+AgNO3 k) AgNO3+NH3 l) NH3+CuSO4. Along the way‚ observations were made pertaining to the reactions witnessed. This experiment concluded
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properties of five common acids used in industry. Give some examples of the typical uses of each. 4. Although HCl(aq) exhibits properties of an Arrhenius acid‚ pure HCl gas and HCl dissolved in a nonpolar solvent exhibit none of the properties of an Arrhenius acid. Explain why. - HCl(g) consists of covalently bonded molecules that don’t ionize. Nonpolar solvent molecules don’t attract HCl molecules to cause them to be ionized. 5. a. What distinguishes strong acids from weak acids? - Strong acids
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Varying the Concentration of 1.0 M HCl | | | | |Concentrations | | |# Drops |# Drops |# Drops |Initial | |# Drops |# Drops |# Drops |Initial |Initial |Final |Final |Reaction Time (sec) |Reaction | |Well # |HCl |Water |Na2S2O3 |HCl |Na2S2O3 |HCl |Na2S2O3 |Trial 1 |Trial 2 |Avg
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of Calcium Hydroxide Used (v/cm3) +0.1 cm3 1 38.65 47.10 8.45 10.0 2 17.55 26.00 8.45 10.0 3 26.00 34.55 8.55 10.0 4 34.55 43.00 8.45 10.0 5 14.15 27.70 8.55 10.0 *there is an assumption that there isn’t an uncertainty for HCl solution* Balanced equation for hydrochloric acid and calcium hydroxide: Ca(OH)2 + 2HCl → CaCl2 + 2H2O Qualitative Data: The dark pink color the indicator gave it immediately vanished after a specific amount of Hydrochloric Acid was added by titration
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secondary alcohols will react with HCL and KmnO4‚ and the tertiary alcohol wont react with either HCL nor KMnO4 due to the location of the OH. The carbon that is bonded to the OH in both primary and secondary still has one or two Hydrogen atoms to undergo reactions‚ but the carbon in the tertiary alcohol do not have any Hydrogen to undergo reactions with. Materials: refer to the handout. Procedure: refer to the handout. Observation: Alcohol | Reaction with HCL | Reaction with KMnO4
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Objective: To study the affect of pH on a food preservative. Chemical Equation: C6H5COONa + HCL ------ C6H5COOH + NaCl Procedure: This experiment was started with a clear solution of sodium benzoate and HCl was added to it‚ ultimately producing benzoic acid. First‚ .3395 g of sodium benzoate was weighed‚ then it was dissolved in water‚ causing it to disassociate into ions. Next‚ 3M of HCl were added drop wise to the solution until it reached a pH of 2‚ thus introducing the hydronium ion
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NaOH solution. 2. Record volume. 3. Measure out between 20 milliliters and 40 milliliters of the unknown HCl solution. 4. Record volume. 5. The amount of unknown HCl is then added to the 100-milliliter Erlenmeyer flask. 6. Add two drops of the indicator‚ phenolphthalein‚ to the acid in the flask. 7. Using the slider on the right hand side‚ add NaOH to the HCl in the Erlenmeyer flask (This action is known as titrate). Add the indicator until the color of the indicator turns
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