5._NH,OH + HC;H;O2 ---> H2O + NH,C;H3O2 Wk. Elect. wk. Elect. ionic, sol. IONIC: NET IONIC: 6. H;SO, ---> H;O + (NH.)2SO4 + HO'HN Wk. Elect. str. Elect. ionic, sol. IONIC: NET IONIC: 7. _MgCl2 ----> Mg(OH)2 + NH.CI + HO'HN Wk. Elect. ionic, sol. ionic, insol. ionic, sol. IONIC: NET IONIC:
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- 2) You are tasked with determining the barium content of a sample containing barium nitrate mixed with rubidium nitrate. The sample is weighed, dissolved into 50.0mg water, and treated with xs 0.500M sodium sulfate. The acid fully ionizes in this experiment. A white precipitate forms which is washed, filtered, and weighed multiple times, according to the data given below: Mass of sample 0.425g Mass of thoroughly dried filter paper 1.462g Mass of precipitate+filter after 1st drying 1.755g Mass of precipitate+filter after 2nd drying 1.699g Mass of precipitate+filter after 3rd drying 1.698g2) You are tasked with determining the barium content of a sample containing barium nitrate mixed with rubidium nitrate. The sample is weighed, dissolved into 50.0mg water, and treated with xs 0.500M sodium sulfate. The acid fully ionizes in this experiment. A white precipitate forms which is washed, filtered, and weighed multiple times, according to the data given below: Mass of sample 0.425g Mass of thoroughly dried filter paper 1.462g Mass of precipitate+filter after 1st drying 1.755g Mass of precipitate+filter after 2nd drying 1.699g Mass of precipitate+filter after 3rd drying 1.698g A] for the chemical reaction that occurs forming the precipitate: (i) write the balanced net-ionic equation for the reaction (ii) explain why the net-ionic equation optimally represents the processYou have prepared 1.000 M of NaOH solution. To determine the accuracy of the solution you prepared you have carried out two titration trials. Calculate the actual concentration of NaOH solution you prepared for each titration trials, and the average concentration. All your final answers should be reported to 4 significant figures. Trial 1: Weight of KHP = 5.0320 g MW(KHP) = 204.2 g/mole NaOH titrant volume = 24.40 ml 2. Trial 2: Weight of KHP = 5.0123 g MW(KHP) = 204.2 g/mole NaOH titrant volume = 24.34 ml Calculate the average concentration of Trial 1 and 2.
- The following volumes of 0.000300 M SCN- are diluted to 15.00 mL. Determine the concentration of SCN- in each sample after dilution. These values will be used during the experiment. Sample 0.000300 M SCN- (mL) [SCN-] (M) 1 1.50 2 3.50 3 7.00 4 10.00The purity of KHP was determined by first weighing KHP using weighing by difference. and the weighed sample was titrated with NaOH solution. Calculate the % purity of the KHP sample given the following data. Express your answer in 2 decimal places. No need to include the unit. I need anwer asap please show solution this is analytical chemistryLe Simple Markup A Previc Show Markup A Next Delete Previous Next Eraser Pen Comments Comment New Show Ink Track Accept Reject Comment Changes Reviewing Pane Comments Tracking Changes 4.Suppose you run a titration of an acid yourself. You do it three times be- tween an acid and sodium hydroxide solution. Here is some data: Average volume of sodium hydroxide solution delivered: 9.10 mL Concentration of sodium hydroxide standard solution: 0.1010 M Average mass of acid solution: 9.555 g The average volume of sodium hydroxide solution is the average of three titra- tions. In other words, you did the experiment three times and took an average. The same goes for the average mass of the acid. You ran the experiment three times and the average mass of the acid solution is given for those three titra- tions. The sodium hydroxide solution was standardized and the concentration is given. Show your step-by-step calculations for this experiment to find the mass per- cent of acid in the solution.…
- A 29.1 mg food sample containing nitrogen was digested according to the Kjeldahl method and the evolved ammonia was absorbed in 22 mL of 0.1 N of HCl solution. 15.5 mL of 0.1 M NaOH solution for complete neutralization. Calculate the total nitrogen content in this sample.B. Determining the Composition of a Mixture of Sodium Chloride and Sodium Nitrate Partner I Prepare a solution of sodium chloride + sodium nitrate and indicator. Obtain a dropper bottle of potassium chromate (indicator) solution. To a clean and dry 125 mL Erlenmeyer flask, add about 40 mL of water and 8 drops of indicator solution. Weigh out approximately 0.05 grams of sodium chloride + sodium nitrate solid and record its exact mass. Dissolve the solid in the solution from step 1, stirring with a stirring rod to ensure complete dissolution. Determine and record the total mass of the Erlenmeyer flask and solution, noting the balance that you use to weigh. Rather than measuring the volume of silver nitrate solution added as in Part A, we will measure the mass of titrant added and make use of the weight-percentage concentration of silver nitrate in calculations. Prepare the silver nitrate solution. Obtain about 15 mL of 1.70% w/w silver nitrate solution in a 50 mL beaker. Designate a…Hi, this is a titration problem and I am experiencing trouble in calculating for the answer though it's already given. I need help, thank you. Andrew dissolved 10.00 grams of an iron ore sample in 5.00 L of acid to produce a stock solution. Josh ran a trial of the analytical procedure on the stock solution, but found the solution was too concentrated to be used. So Josh prepared a 1:250 dilution of the sample solution, and, after running the analytical procedure successfully, found the solution contained 1.62 x 10-5 mol/L Fe2+ (aq). What is the mass of iron in the meteorite sample? Answer: 1.13 g Fe
- 1. Precipitates are produced from a chemical reaction. Give at least 3 types of appearances or textures of precipitates. 2. Determine the strength of a Test Solution in millimolar concentration. [express answer up to 4 decimal places] 3.What gas (chemical name) is evolved when the odor observed is sour-like, and not too irritating to the nose? 4.Give at least 8 manifestations or observable results after a chemical reaction has completed.A. A Set of Standard Solutions Data Analysis, A 16a mmin 16b B. Determination of max Identify the metal ion for analysis on the Report Sheet. 1. Prepare a stock solution. a. Prepare 100 mL of a 0.10 M stock solution. To do this, you will need to know the formula of the Cu²+, Ni²+, or Fe³+ ion-containing salt in order to calculate the mass of salt for its preparation. See Prelaboratory Assign- ment question 2a. Show a similar calculation for your selected metal ion on the Report Sheet. Measure the mass of the salt (±0.001 g). b. Transfer the salt to a 100-mL volumetric flask, half-filled with 0.01 M HNO3, add the appropriate complexing agent (see Table 35.1), and then dilute to the mark with 0.01 M HNO3. Record on the Report Sheet the exact molar concentration of the stock solution. Table 35.1 Volume of Complexing Agent for Stock Solution Preparation Metal Ion Volume of Complexing Agent Cu²+ 10 mL of conc NH, Ni²+ 10 mL of conc NH; Fe³+ 20 mL of 0.1 M NASCN 2. Prepare the standard…3 An analyst weighed 0.5002 g of Apple Leaves Standard Reference Material (SRM#1515) to determine cadmium levels. The digestate was completed to the 25.0358 mL mark with distilled water. to. a. 1Indicate the Cd concentration as it appears on the Certificate of Analysis for this control. b. If the analyst recovered 92.6%, calculate the concentration (in ppb) of Cd in the solution.