of the water removed is .51 grams. The water of hydration was calculated to be about 2. Based on these measurements‚ the empirical formula of the hydrate is BaCl2 • 2H2O. This means that for every mole of BaCl2‚ there is about two moles of water. The weight percentage of water to hydrate is about14.75%. This means that in the total mass of BaCl2 • 2H2O‚ water makes up about 14.75%. However‚ labs such as this may not be accurate‚ since there are many places where error could have occurred. For example
Premium Water Chemistry
Casey and Robert Tatz‚ Hayden McNeil Publishing‚ 2010 Report Sheet See attached report sheet. Report Questions 1. Explain how your calculated value for percent sulfate would be affected if: a. Insufficient BaCl2 is added. In the case that insufficient BaCl2 would be added‚ some SO4 (sulfate) molecules from the sample would have remained in the solution without precipitating and therefore‚ a smaller than the actual amount of sulfate would have been determined. b. Addition
Premium Chemistry Solubility Water
Sodium sulphide forms H2S gas with rotten egg smell and also turns lead acetate paper silvery black. c)Sodium sulphide (Na2S)& Sodium sulphate (Na2SO4) using barium chloride(BaCl2) Ans: Sodium sulphate (Na2SO4) forms white ppt. with barium chloride (BaCl2)‚ Sodium sulphide (Na2S) does not form any ppt. with barium chloride(BaCl2) d)Sodium chloride (NaCl)&Sodium nitrate (NaNO3) using conc. Sulphuric acid Ans: Sodium chloride (NaCl) forms HCl gas with conc. Sulphuric acid
Free Sodium hydroxide Ammonia Sodium chloride
measured mass of the unknown salt in water. Next you will add an excess of aqueous barium chloride to the aqueous solution of the unknown salt. This will result in the precipitation of the sulfate as barium sulfate. BaCl2(aq) + M2SO4(aq) →BaSO4(s) + 2 MCl(aq) (assuming +1 cation) BaCl2(aq) + MSO4(aq) →BaSO4(s) + MCl2(aq) (assuming +2 cation) The barium sulfate precipitate is collected by filtration‚ ignited and weighed. The number of moles of sulfate can be determined from the mass of the barium
Premium Solubility Filter paper
NiCl2 or NiSo4 cuz Ni turned blue in presence of ammonia (i think only periods 1 and 2 can use this) ○ Was solution 3 soluble or insoluble in Bacl2 and Agno3? That can help us decide whether its cl2 or so4. bacl was precipitate ■ precipitate in bacl2 and naoh ■ Unknown 4 ● CuSo4 ○ bacl2 precip means so4 ○ blue color means copper ○ also paperclip looked copper colored when left in this solution ● Unknown 5 ● NH4NO3 or NH4Cl ○ nh4cl most likely
Premium Solubility Sodium chloride Sodium hydroxide
to a minute. Promptly centrifuge and transfer the heated supernate into a fresh test tube. Replicate the process a few more times and integrate the supernate. retain the precipitate for the testing of Ag+ if there was any. lastly add 3 drops of 1M K2CrO4 to the supernate. When a yellow precipitate forms then that confirms the presences of Pb Identification of Ag+
Premium Chemistry Bacteria Water
(PbNO3) and potassium chromate (K2CrO4) solutions B. Reaction between potassium permanganate (KMnO4) and oxalate ion (C2O42-) C. Iodine clock reaction A. REACTION BETWEEN LEAD NITRATE AND POTASSIUM CHROMATE SOLUTIONS Lead nitrate reacts with potassium chromate to form yellow lead chromate precipitate and aqueous potassium nitrate. The formation of a yellow precipitate indicates the completion of the reaction. The reaction is extremely fast. Pb(NO3)2 (aq) + K2CrO4 (aq) → PbCrO4 (s) + KNO3
Premium Iodine Chemical reaction Chemical kinetics
two are opposite ions that attract to one another. In this lab research‚ I learned that the following reaction will happen: lead nitrate + potassium chromate à potassium nitrate + lead chromate‚ the balanced chemical reaction is: Pb (NO3)2 + K2CrO4 --> 2 KNO3 + PbCrO4 Procedure Materials: - (1) 100ml Beaker - (1) 50 ml(s) of potassium chromate 1M solution - (1) 50 ml of lead (II) nitrate 1M - (1) 250 mL Erlenmeyer flask - (1) Buchner funnel - (1) Test tube Procedure: 1. Gather
Premium Ion Chemistry Potassium
I. Experiment 3: SEPARATION TECHNIQUES II. Objectives: * To learn different methods and techniques of separating components of mixtures * To appreciate the importance of such separation techniques * To apply different methods and techniques in separating components of mixtures III. Results and Observations Separation of components with different solubilities * AMMONIUM CHLORIDE‚ SODIUM CHLORIDE‚ SAND the wt. of mixture with evaporating dish after 1st heating is?? g. And after
Premium Solubility Liquid Evaporation
the gravimetric analysis technique. The solution of Na2SO4 (0.5 M) and BaCl2 (0.1 M) were chosen in this experiment. The equation was used: Na2SO4 (aq) + BaCl2 (aq) → BaSO4 (s) + 2 NaCl (aq). However‚ in this reaction‚ cation Ba2+ and anion (SO4)2- play the main roles to form precipitated BaSO4: Ba2+(aq) + (SO4)2(aq) = BaSO4 (s).Assuming that 0.200g BaSO4 (s) were produced in this experiment‚ the volume of Na2SO4 and BaCl2‚ needed to form 0.200g BaSO4‚ were determined by using the stoichiometry
Premium Solubility Stoichiometry Precipitation