acid NaHCO3 + HCl → NaCl + CO2 + H2O a) Unknown mixture of NaCl and NaHCO3 Mass of unknown mixture (NaCl + NaHCO3) | 3 g | Mass of HCl | 30 .31g | Mass of products ( NaCl + H2O ) | 26.98 g | Calculate mass of CO2 | 6.33g | Calculate mass of NaHCO3 | 12 .1 g | i) Calculation : Mass of CO2 = [Mass of unknown mixture (NaCl + NaHCO3) + Mass of HCl ] – [Mass of NaCl + H2O] = (3 g + 30.31 g) – 26.98 g = 6.33g Mass of NaHCO3 : 6.33 g CO2 * 1 mol CO2 44.10 g CO2 * 1 mol NaHCO3 1 mol
Premium Hydrochloric acid Sodium carbonate Sodium bicarbonate
2013 Abstract The analyte used is the soda ash which is titrated with an HCl titrant‚ standardized by Na2CO3. The indicators used are phenolphthalein for basicity and methyl orange for acidity. The two volumes of the titrant are then used to calculate percent composition of soda ash analyte. At the end of the experiment‚ the calculated average percent by mass of Na2CO3 is 4.92% and the average percent by mass of NaHCO3 is 5.07%. Introduction Soda ash is the common name for sodium carbonate
Premium Titration Sodium hydroxide Hydrochloric acid
better understanding of chemical stoichiometry. We are going to be reacting sodium bicarbonate (NaHCO3) and sodium carbonate (Na2CO3) with hydrochloric acid (HCl). To start off the mass of two unknown substances (being the sodium bicarbonate and sodium carbonate) will be taken. We will need to construct balanced equations for both of the reactants with the HCl and use this to guide us to figure out how much HCl will be needed to react with each of the unknown substances. When this part is through we will
Premium Hydrochloric acid Sodium chloride Chlorine
the following mixture by double indicator method: 1. NaOH(aq) and Na2CO3(aq) 2. NaHCO3(aq) and Na2CO3(aq) Introduction Consider a mixture of NaOH(aq) and Na2CO3(aq). Reaction between HCl(aq) and Na2CO3(aq) takes place in two stages: HCl(aq) + Na2CO3(aq) ⎯→ NaHCO3(aq) + H2O(l) …………………. (1) HCl(aq) + NaHCO3(aq) ⎯→ NaCl(aq) + CO2(g) + H2O(l) …………. (2) While that between HCl(aq) and NaOH(aq) completes in only one step: HCl(aq) + NaOH(aq) ⎯→ NaCl(aq) + H2O(l) ……………….………. (3) Solution mixture of reaction
Free PH indicator Titration PH
titrations of NaHCO3 and NA2CO3 with HCl. A chemical reaction is a process that involves rearrangement of the molecular or ionic structure of a substance‚ as opposed to a change in physical form in a nuclear reaction. Titration is when a measured amount of solution of unknown volume is added to a known volume of a second solution until the reaction between them is complete. The objective of this experiment is reacting sodium bicarbonate (NaHCO3) and sodium carbonate (NaCO3) with hydrochloric acid (HCl) to
Premium Hydrochloric acid Sodium carbonate Chlorine
analyte was the soda ash sample and the titrant was the HCl which was standardized by a primary standard of known purity‚ the sodium carbonate. Standardization is the process in which the concentration of solution is accurately determined. A sample of sodium carbonate with 99.9% purity was dissolved in boiled water and titrated with HCl. Then‚ a sample of soda ash was dissolved in boiled water and then‚ titrated. In a this reaction of HCl with carbonate‚ the following reactions will take place:
Premium PH Titration PH indicator
Introduction: A balanced chemical equation has reactants and product that has to represent a formulae. The amount of each element‚ number needs to be the same in either side of the equation. (E.g.‚ HCl(aq)+NaHCO3(s) reacts to produce NaCl(aq)+H2O(I)+CO2(g)‚ this is the equation given for this lab). This help us view the study of Law of Conservation of Mass‚ when either side of equation is equally balanced. The calculation for formula mass helps determine if you need to convert grams to a particular
Premium Hydrochloric acid Evaporation Chemistry
4. To determine amount of heat release in the reaction. Results: Part 1: Thermal Decomposition of NaHCO3 Materials Mass (g) Clean and dry test tube 15.1632 Clean test tube + NaHCO3 17.1647 Amount of NaHCO3 added 2.0015 After heated test tube + NaHCO3 16.4500 Amount of solid product (NaHCO3 + any unreacted NaHCO3) 1.2868 Part 2: Titration of Na2CO3 with Hydrochloric acid (HCl) First Reading Second Reading Third Reading Initial
Premium Chemical reaction Chemistry Chlorine
Joshua McMahon IB Chemistry Matt Chase 3A 11/5/14 Finding the Molar Enthalpy Change of sodium bicarbonate by using Hess Law Research Question By using Hess’ Law‚ can the Molar Enthalpy Change of sodium bicarbonate be calculated? Hypothesis If we are attempting to determine the enthalpy change of the thermal decomposition of Sodium Bicarbonate‚ then Hess’s Law will be will be the most effective. Introduction Sodium bicarbonate‚ more commonly known as baking soda‚ has many uses in todays
Free Thermodynamics Temperature Enthalpy
Masses Empty Dish NaHCO HCl+NaCO3 Final (Dish and Salt Product 24.35 (grams) 10.06 (grams) 40.06 (grams) 31.52 (grams) 2. Write the complete balanced equation for the reaction that occurred in this lab. Hint: H2CO3 is not a final product of the double-replacement reaction; it breaks down (decomposes) immediately into two products. (3 points) NaHCO3 + HCl → CO2 + H2O + NaCl 3. The NaHCO3 is the limiting reactant and the HCl is the excess reactant
Free Stoichiometry Yield Water