You are making ampicillin plates. Before pouring the plates, you add 2 mL of 10 mg/mL to the 400-ml bottle of LB agar that you use to pour the plates. What is the final concentration of the ampicillin in the plates? Express your answer as µg/mL. Show your work.
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- 50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution. Information of stock solution - molar mass- 534.3g/mole 0.587g in MilliQTable 1: Temp vs. solubility data of ammonium chloride. Test tube g NH4Cl/10 mL H2O Crystallization temp. (ºC) 1 1.0 g/10 mL H2O 10 oC 2 1.8 g/10 mL H2O 20 oC 3 2.9 g/10 mL H2O 40 oC 4 3.8 g/10 mL H2O 65 oC 5 4.4 g/10 mL H2O 95 oC Use the table to plot a solubility curve for ammonium chloride on the graph provided below. For the best fit line, use a smooth curve. "Mass of Solute per 100 mL of H2O," should be written on the y-axis (use increments of 2g for every box). "Temperature (°C)" should be written on the x-axis (use increments of 10 °C for every 2 boxes).You have a 20% stock of NaCl, a 30% stock of K2HPO4, 2.5 M NH4Cl and 10 mg/ml stock of ampicillin. a. How many grams of NaCl would you need to weigh out to make up 150 ml of a solution?b. You will be preparing 300 ml of media. You need to dilute this 20% stock of NaCl, the 30% stock of K2HPO4, the 2.5 M NH4 how much stocks you need to add. Fill in the table below. Stock Calculate Final Concentration needed ml added20% NaCl 1.5% ? 30% K2HPO4 2% ? 2.5 M NH4 Cl 0.1M ? 10 mg/ml ampicillin water 0.05 mg/ml ? water To 300 ml ?
- 15. You are given a series of 10 tubes. In the first is placed 9 milliliters of saline. In each of the others is placed 5 mL of saline. One milliliter of serum is added to the first tube. Five milliliters from this tube are transferred to the second tube, and 5 ml are transferred throughout the remaining tubes. Discard the last 5ml transferred. Give the following: a. Tube dilution for tubes 1 and 6 b. The solution dilution for tubes 1,4, and 7 c. The amount of serum present in tube #3 after transfer.A student, trying to standardize NBS solution using a standard Vitamin C solution (220 mg/L), obtained data that was obviously incorrect. They realized their mistake when they noticed the standard Vitamin C solution was dated 8/04. What was their mistake and explain why?A 1 mL sample of glycogen was calculated to contain 21 µmol (micromole) glucose. To 1 mL of this sample was added 2 mL of 2 M HCl. It was then hydrolysed by boiling the solution for 15 minutes. After boiling the hydrolysate was cooled and made up with H2O to a final volume of exactly 10 mL. The glucose was measured in this solution and found to have a concentration of 340 µg/mL (microgram/milliliter). i) Calculate the mass (mg) of glucose in the 10 mL of hydrolysate. As the 1 mL of glycogen sample was made up to a final volume of 10 mL, this mass of glucose was produced by the hydrolysis of the original 1 mL glycogen sample. ii) Calculate the amount (µmol) of glucose produced by the hydrolysis of the glycogen sample. iii) Calculate the purity of the glycogen used in the sample as % Purity = (moles of measured glucose/ moles of calculated glucose in glycogen) *100 iv) state your answer in a complete sentence. Show your working out such that the marker can easily understand it.…
- A 1 mL sample of glycogen was calculated to contain 35 µmol (micromole) glucose. To 1 mL of this sample was added 2 mL of 2 M HCL. It was then hydrolysed by boiling the solution for 15 minutes. After boiling the hydrolysate was cooled and made up with H2O to a final volume of exactly 10 mL. The glucose was measured in this solution and found to have a concentration of 570 µg/mL (microgram/milliliter). i) Calculate the mass (mg) of glucose in the 10 mL of hydrolysate. As the 1mL of glycogen sample was made up to a final volume of 10 mL, this mass of glucose was produced by the hydrolysis of the original 1 mL glycogen sample. ii) Calculate the amount (µmol) of glucose produced by the hydrolysis of the glycogen sample. iii) Calculate the purity of the glycogen used in the sample as % Purity = (moles of measured glucose/ moles of calculated glucose in glycogen) *100 iv) state your answer in a complete sentence.A protocol calls for 1 liter of solution that is 1.5 % (w/v) NaCl, 5mM Tris (pH 8.0), 10% (w/v) Carnation Instant Milk (we really do use this in lab!), and 0.03% (v/v) Tween-20 detergent. How do you make this solution?Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…
- Pretend you are making dilutions using a 20-mg/dL stock standard solution of uric acid. Complete the table to indicate preparation of various concentrations. Concentration (mg/dL) Stock Standard (mL) Distilled H2O Total Volume of Dilution (mL) 0 0.0 5.0 5.0 2.5 5.0 5.0 5.0 7.5 5.0 10.0 5.0 12.5 5.0 20.0 5.0 0.0 5.0In the phosphate analysis of a wastewater sample, 30.00 mL of the original sample was taken and diluted with 120.00 mL deionized water. The diluted sample was found to have a phosphate content of 25.5 ppm. What is the phosphate content (in ppm) of the original wastewater sample?2. An 88-pound patient will be receiving aztreonam 30 mg/kg (MAX 1 gram) in 100 mL D₁0W. MWaztreonam = 435.43 g/mol General Structure: aztreonam a. If you have aztreonam 40 mg/mL in stock, calculate the appropriate volume, in milliliters, of the stock solution the patient should receive. b. Fill in the values on the table.