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What is 300 simplified as a radical?
The number 300 can be simplified as a radical by factoring it into its prime factors: (300 = 100 \times 3 = 10^2 \times 3). Therefore, the square root of 300 can be expressed as ( \sqrt{300} = \sqrt{100 \times 3} = \sqrt{100} \times \sqrt{3} = 10\sqrt{3}). Thus, the simplified form of 300 as a radical is (10\sqrt{3}).
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.
How much pure alcohol is in 300 liters of 30 percent alcohol solution?
To find the amount of pure alcohol in a 300-liter solution that is 30 percent alcohol, you can multiply the total volume by the percentage of alcohol. This calculation is as follows: 300 liters × 0.30 = 90 liters. Therefore, there are 90 liters of pure alcohol in the 300-liter solution.
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.
What is 300 simplified as a radical?
The number 300 can be simplified as a radical by factoring it into its prime factors: (300 = 100 \times 3 = 10^2 \times 3). Therefore, the square root of 300 can be expressed as ( \sqrt{300} = \sqrt{100 \times 3} = \sqrt{100} \times \sqrt{3} = 10\sqrt{3}). Thus, the simplified form of 300 as a radical is (10\sqrt{3}).
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?
Use M1V1=M2V2 Where M is the concentration (5.5 m for M1 and 1.2 m for M2) and V is volume V1 is 300 ml and V2 is your unknown. Using this calculation for other questions be sure that units are all the same. So all molarities and all mL in this example.
What mass of MgSO4 7 H2O is required to prepare 300 mL of a 0.529 M MgSO4 solution?
To prepare a 0.529 M MgSO4 solution, you first need to calculate the moles of MgSO4 required for 300 mL (0.300 L) of solution: Moles of MgSO4 = Molarity × Volume = 0.529 mol/L × 0.300 L = 0.1587 mol. Next, since MgSO4·7H2O is the hydrated form, its molar mass is approximately 246.47 g/mol. Therefore, the mass needed is: Mass = Moles × Molar Mass = 0.1587 mol × 246.47 g/mol ≈ 39.06 g of MgSO4·7H2O.
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.
