Imagine you collected a master batch (undiluted) wastewater sample as shown in the illustration below. The total mass of lead (Pb) found in 300 mL of a two-fold diluted master sample was 1.65 µg Calculate the amount of Pb in the master batch sample of the wastewater in ppb. Enter numerical values rounded to one significant figure without units. Volume of solution: 1 L Mass of solution: 1.1 kg

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Please help me answer questions 1 and 2. (Questions attached below) 1. When you arrive at the lab, 2.0 M H2SO4(aq) and 2.0 M HC2H3O2(aq) will be present. Youwill need to dilute these solutions using beakers and graduated cylinders from your drawerand DI water.i. Calculate the volume of the 2.0 M HC2H3O2(aq) and DI water needed to create 50.0 mLof 1.05 M HC2H3O2(aq).ii. Calculate the volume of the 2.0 M H2SO4(aq) and DI water needed to create 50.0 mL of0.75 M H2SO4(aq). 2. A 48.33-mL sample of 0.150 M NaBr is titrated into 50.00 mL of 0.145 M AgNO3. Bothsolutions had the same initial and final temperatures. The reaction occurred in a calorimeterwith a known heat capacity and produced 1546.03 J of heat.i. Write a balanced equation that is occurring.ii. Determine the theoretical yield of the solid.iii. Calculate the enthalpy of the reaction (kJ/mole of precipitate).

A student prepared a standard copper solution by combining 2.63 mL of stock 0.270 mol/L copper(II) sulfate solution with 6.37 mL of water. What is the molar concentration of Cu2+ in this solution? Give your answer in in decimal format. When entering units, use proper abbreviated units with proper capitalization.

An analytical chemist weighs out 0.087 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 5.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.

A solution is prepared by dissolving 72.91 g of CdCl2 (MM = 183.317) in enough water to make 158.95 mL of solution. If the density of the solution is 1.556 g/mL, what is the molarity of the chloride ions, Cl-(aq), in solution? Report your answer using two decimal places.

Please help me with this one Sugar is the solute and water is the solvent. The drink mix will be considered negligible and is added simply for the visualization of dilution results. Calculate the concentration of sugar in this solution using the volume percent equation. Refer to the background for sample calculations. For the purpose of this exercise, it can be assumed that the weight of the drink mix is 0.00 g. The volume of the solution is 3 and 1/3 cups. Convert to metric units, then calculate and record the volume percent in Data Table 1 (Note that 1 cup = 236 mL). Volume % = Volume of Solute/ Volume of Solution × 100%

Most analytical machines used in science can either measure absorbance of light, like the spectrophotometers used BioZ 151 and 152 labs, or can measure change in electrical conductance. In order to convert things like absorbance values into concentration data, a linear regression is used. In order to determine nitrite concentration in water samples, nitrite is reacted with several chemicals to produce a purple color. The absorbance of the solution is measured from known amounts of nitrite to produce a standard curve to analyze samples. Use the data in the provided table, or from the linked spreadsheet to make a graph and perform a linear regression using treadline. mg/L NO3 Absorbance 0 0.1 0.3 0.5 0.7 o 0.183 0.542 0.914 1.298) 1.61) In order for this to work, samples must be diluted prior measurement so that the concentration falls within the range of the standard curve. If a sample underwent a 30 dilution, and produce an absorbance value of 0.953, what is the resultant concentration…

In the laboratory, a student adds 14.0 g of silver nitrate to a 375 mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of silver nitrate, the silver ion and the nitrate ion in the solution.

In the laboratory, a student dilutes 10.1 mL of a 7.85 M hydroiodic acid solution to a total volume of 125.0 mL. What is the concentration of the diluted solution? Concentration=____M