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What is simplify radical terms 300?
I think you want: √300 = √(100 x 3) = √100 x √3 = 10√3
What quantity of a 80 percent acid solution must be mixed with a 30 percent solution to produce 300 mL of a 40 percent solution?
Let Q be the quantity of 80% solution required then (300 - Q) is the quantity of 30% solution as together the two solutions must equal 300. Then, [80 x Q] + [30 x (300 - Q)] = [40 x 300] 80Q + 9000 - 30Q = 12000 50Q = 3000 Q = 60...........which means (300 - Q) = 240 60ml of 80% acid solution + 240ml of 30% solution produces 300ml of 40% solution.
Can 16 go into 300 evenly?
No, 18.75 is the solution.
What is the solution of 300 means between 100 and 400?
The statement "300 is between 100 and 400" is equivalent to: 100 < 300 < 400 Or the equivalent: 300 > 100 AND 300 < 400. If you check these statements and see that they are true, then 300 is between the two numbers.
Create an equation whose solution is 150.?
You could do this by staring with the answer:150x2 = 300; 300+72 = 372; 372/6 = 62.(2x + 72)/6 = 62
How would you prepare a 300 ml of a 0.1 M Na CL solution from a solid Na CL solution and water?
You prepare a solution by dissolving a known mass of solute into a specific amount of solvent. In solutions, M is the molarity, or moles of solute per liter of solution. For 300 ml of a 0.1 M Na CL solution from a solid Na CL solution and water you need water and sodium chloride.
How many moles of potassium hydroxide are required to prepare 300 mL of 0.250 M solution?
To calculate the moles of potassium hydroxide needed, use the formula: moles = molarity * volume (in liters). First, convert 300 mL to liters (0.3 L). Then, moles = 0.250 mol/L * 0.3 L = 0.075 moles of potassium hydroxide needed to prepare the solution.
What is the reduced radical form of 300?
300 = 100*3 So sqrt(300) = 10*sqrt(3)
What is the square root of 300 in radical form?
10 sqrt(3)
How many moles of NaOH needed to prepare 300 mL of a 0.2 m solution of NaOH?
To find the moles of NaOH needed, use the formula: moles = concentration (molarity) x volume (liters). First, convert 300 mL to liters (0.3 L). Then, calculate: moles = 0.2 mol/L x 0.3 L = 0.06 moles. Therefore, 0.06 moles of NaOH are needed to prepare 300 mL of a 0.2 M solution.
What is simplify radical terms 300?
I think you want: √300 = √(100 x 3) = √100 x √3 = 10√3
What quantity of a 80 percent acid solution must be mixed with a 30 percent solution to produce 300 mL of a 40 percent solution?
Let Q be the quantity of 80% solution required then (300 - Q) is the quantity of 30% solution as together the two solutions must equal 300. Then, [80 x Q] + [30 x (300 - Q)] = [40 x 300] 80Q + 9000 - 30Q = 12000 50Q = 3000 Q = 60...........which means (300 - Q) = 240 60ml of 80% acid solution + 240ml of 30% solution produces 300ml of 40% solution.
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How many millilieters of 5.5 m naoh are needed to prepare 300 ml of 1.2 m naoh?
To prepare the 1.2 M NaOH solution, you need to dilute the 5.5 M NaOH solution. By using the formula C1V1 = C2V2 (where C1 is initial concentration, V1 is initial volume, C2 is final concentration, and V2 is final volume), you can calculate the volume of the 5.5 M NaOH solution needed to make 300 ml of 1.2 M NaOH solution. In this case, V1 would be the volume of the 5.5 M NaOH solution you need to calculate.
How much 95 percent alcohol must be used to prepare 1000 ml of 70 percent alcohol?
To prepare 1000 ml of 70% alcohol solution, you would need to mix 700 ml of 95% alcohol with 300 ml of water. Starting with a base of 95% alcohol ensures that the final solution will be at least 70% alcohol.
What is the exact value answers in degrees of two cos x minus radical three equals zero?
30 degrees explanation 2Cosx-radical 3=0 Then 2cosx=radical 3 and cos x=(radical 3)/2 Now remember that cos 300 is (radical 3)/2 from the 30/60/90 triangle. So the answer is 30 degrees.
How do you prepare 300 micro molar H2O2 using 3.0 percent H2O2?
To prepare a 300 µM solution of H2O2 from a 3.0% H2O2 stock solution: Calculate the molarity of the 3.0% solution by dividing the percentage by the molar mass of H2O2. Then, use the formula C1V1 = C2V2, where C1 is the molarity of the stock solution, V1 is the volume needed to prepare, C2 is the desired molarity (300 µM), and V2 is the final volume of the solution (usually in mL). After solving for V1 (volume needed to prepare), measure this volume from the stock solution and dilute it to the final volume with the appropriate solvent (usually water).
