Prepare 100 μL of 10.0 mM hydrolyzed sucrose in 10.0 mM acetate pH 4.8 as a standard, in a 1.5 mL microcentrifuge tube, also incorporating 5.00 μL of 5.0 mM tris pH 7.4 within the 100 μL volume. Using a stock solution of 20.0 mM sucrose substrate in 10.0 mM acetate, calculate the volumes of hydrolyzed sucrose, acetate, and dH2O.
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Prepare 100 μL of 10.0 mM hydrolyzed sucrose in 10.0 mM acetate pH 4.8 as a standard, in a 1.5 mL microcentrifuge tube, also incorporating 5.00 μL of 5.0 mM tris pH 7.4 within the 100 μL volume. Using a stock solution of 20.0 mM sucrose substrate in 10.0 mM acetate, calculate the volumes of hydrolyzed sucrose, acetate, and dH2O.
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- (A) if both sentences are true,(B) if both sentences are false,(C) if the first sentence is true but the second is false, and(D) if the first sentence is false but the second is true. 1. In the Winkler Titration Method, sodium thiosulfate is standardized against a known concentration of magnesium iodate. The normality (N) of a solution is always equal to its molarity (M). 2. In the experiment on determining the dissolved oxygen concentration of a water sample, the compound used to acidify the sample was hydrochloric acid. An acidic solution will have a pH greater than 7. 3. Radioactive wastes, like uranium, must be handled and disposed of according to special regulations designed to protect people and the environment. Nuclear power plants produce too much greenhouse gases due to the burning of uranium.Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate)To determine the Kgp of barium oxalate at 12°C, a 100.0 mL saturated solution was prepared by adding the solid in distilled water maintained at 12°C until it no longer dissolves. The solution was filtered and from this, a 10.0 mL aliquot of the filtrate was drawn. It was found out that 10.70 mL of 5.60 x 104 M HCI was used to reach the endpoint. Given that two moles of HCl react for every mole of dissolved oxalate during the titration, determine the amount of dissolved oxalate in the titration flask (in mol/L). Do not include the unit in your answer below. For those who will be using scientific notation, please follow the format below: Example: 0.00487 -> 4.87E-3 58000 -> 5.8E+4
- GRAVIMETRIC ANALYSIS The addition of dimethylglyoxime, H2C4H602N2, to a solution containing nickel(Il) ion gives rise to a precipitate: Nickel dimethylglyoxime is a bulky precipitate that is inconvenient to manipulate in amounts greater than 135 mg. The amount of nickel in a type of permanent-magnet alloy ranges between 22% and 38%. Calculate the sample size that should not be exceeded when analyzing these alloys for a nickel.In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the mass of potassium chloride present in the salt sample.Consider the reaction of 75.0 mL of 0.350 M C5H5N (Kb = 1.7 x 107⁹) with 100.0 mL of 0.425 M HCI. Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction. 1 U 1 + 4- 2 0₂ H₂O Reset 0 3 □ H 2 4 → C 0 5 6 H3O+ + 6 (s) H* ²+ AWW 4 7 8 7 (1) OH 8 • x H₂O 4+ 9 0 N (g) (aq) 0 Delete
- In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the mass of potassium nitrate present in the salt sample.In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate ΔTf for the experiment.A standard solution is prepared by diluting the stock solution and used in chemical analysis for preparing the standard curve. Larutan piawai disediakan dengan melakukan pencairan larutan stok dan digunakan dalam analisis kimia untuk penyediaan lengkuk piawai. A) Illustrate how do you prepare a stock solution of 0.01 g of NaNO2 in one liter of distilled water in laboratory.
- In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride.1. Calculate ΔTf for the experiment.2. Calculate the molality of the solution.3. Calculate the mass of potassium nitrate present in the salt sample.In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride.1. Calculate ΔTf for the experiment.2. Calculate the molality of the solution.3. Calculate the mass of potassium chloride present in the salt sample.In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the molality of the solution.