What mass of BaSO4 (MW=233.4 g/mole) would precipitate if 10.0 ml of a 0.2 M solution of Na2SO4 was added to the 50.0 ml solution.

Suppose you want to measure the amount of glucose in a can of soda. You can use the data generated in this experiment to help you, but what other data would you need to collect in order to measure the concentration of glucose in the soda? In other words, what additional experimental step(s) would you perform? B I U Ꭶ X X, 14▾ A In order to measure the amount of glucose in a can of soda, one would need to prepare a series of standard solutions w/ an unknown concentrations of glucose using the 0.3M of glucose sol'n and DI water. Therefore, the glucose oxidase assay would be performed on each standard sol'n and the result values would also be measured by a spectrophotometer. A standard curve may then be plotted by absorbances and the unknown concentration of glucose. It may also be necessary to adjust the pH of the soda can sample to preform additional steps. Change Submission Submitted. Waiting on graded response. 14) Once you have collected data from the step(s) proposed in the previous…

A solution was prepared by dissolving 0.687 g of sulfur, S, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. (K, = 3.08°C/m and Kf = 3.59°C/m, T, = 118.5°C and T† = 16.60°C) Freezing point: °C Boiling point: °C

An unknown mixture is known to contain only Ba(OH)2 (MW=171.34 g/mole) and NaOH (MW=40.0 g/mole).  If the mixture is known to contain 45% by mass NaOH, and 8.0 grams of the mixture is dissolved completely in 50.0 ml of solution, answer the following.   a).   How many ml of 0.2 M H2SO4 is needed to titrate the 50.0 ml solution to the equivalence point.

You prepare a standard solution of ferrous ammonium sulfate that is 50.0 ppm in Fe. You pipette aliquots of 0.50 mL, 1.00 mL, 2.00 mL, 4.00 mL, 8.00 mL, and 10.00 mL into 100-mL volumetric flasks, add 1 mL of hydroxylamine solution, 3 mL of o-phenanthroline solution, and sufficient citrate to adjust to pH 3-4 as described in your laboratory instructions. After diluting each sample to the 100 mL mark, and allowing time for the color to develop, you record the absorbances shown in the table. The data is a bit scattered. Looks like your pipetting ability could use some improvement. However, you can still use this data as a calibration curve. Plot the data in Excel, obtain a trendline and the equation for the linear regression line. Print the graph with the equation and turn in to your laboratory instructor with your name and section printed at the top. Fe Conc. Absorbance (ppm) 0.50 1.0 2.0 3.0 4.0 5.0 0.210 0.258 0.355 0.492 0.659 0.856 Use this graph to answer the following questions:…

Consider the following solutions:   (i) 400.0 mL of 0.10 M NaCl (ii) 300.0 mL of 0.10 M CaCl2 (iii) 200.0 mL of 0.10 M FeCl3 (iv) 200.0 mL of 0.10 M KBr (v) 800.0 mL of 0.10 M sucrose   Solution (v), the sucrose solution, has the greatest number of ions. Solution (iii), the FeCl3 solution, has the greatest number of ions. Solution (iv), the KBr solution, has the greatest number of ions. Solution (i), the NaCl solution, has the greatest number of ions. Solution (ii), the CaCl2 solution, has the greatest number of ions.

Given: If you weigh out exactly 0.150 g of an unknown substance to be dissolved in the 100.00 mL volumetric flask, and the concentration of Fe(II) in the 50 mL volumetric flask is calculated to be 1.27 x 10-4 M a. what is the mass (in grams) of iron that you would have in a 100.0 g sample of an unknown substance? HINT GIVEN: You are back calculating from the [Fe(II)] in 50.00 mL to [Fe(II)] in 100.00 mL and then determine the grams of Fe(II) in the mass of unknown sample weighed out to place in the 100 mL flask, to finally be able to calculate the mass of iron in 100.0g of sample.   (answer a )

A 2.45 g mixture of BaCl2 and Ba(NO3)2 is dissolved in water.  Excess AgNO3 is added and all of the dissolved chloride ion is precipitated. The resulting precipitate weighs 0.845 g.  Use the following Molar Masses (in g mol−−1) as required: Ba: 137.3 Cl:  35.45 Ag: 107.9 N: 14.01 O: 16.00   What is the mass of Ba(NO3)2 in the original mixture?  Enter a mass accurate to three significant figures.  g

Chemistry Question

A 2.45 g mixture of BaCl2 and Ba(NO3)2 is dissolved in water.  Excess AgNO3 is added and all of the dissolved chloride ion is precipitated. The resulting precipitate weighs 0.845 g.  Use the following Molar Masses (in g mol−−1) as required: Ba: 137.3 Cl:  35.45 Ag: 107.9 N: 14.01 O: 16.00   What is the mass of Ba(NO3)2 in the original mixture?  Enter a mass accurate to three significant figures.