An aqueous solution contains 0.10 M NaOH. The solution is basic. An aqueous solution containing 0.10 M NaOH is basic. Correct answer is C.
NaOH is a strong base, meaning it dissociates completely in water to form Na+ and OH- ions. The OH- ions, also known as hydroxide ions, are responsible for the basic nature of the solution. When hydroxide ions are present in a solution, they can react with hydrogen ions (H+) to form water, which is a neutral compound. This reaction is known as neutralization.
The pH of a basic solution is greater than 7, and in the case of this solution, it is expected to be around 12. This indicates that the solution is highly alkaline. The strength of a basic solution can be determined by measuring the concentration of hydroxide ions. In this case, the concentration of hydroxide ions is 0.10 M, which is relatively high.
The dilution of a solution refers to the amount of solute (in this case, NaOH) present in a given volume of solvent (in this case, water). A solution is considered dilute if the amount of solute is relatively small compared to the volume of solvent. Since the concentration of NaOH in this solution is 0.10 M, it is not considered a very dilute solution.
Finally, the color of a solution is not directly related to its basicity or acidity. However, some substances, such as indicators, may change color depending on the pH of a solution.
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which is usually the beat stage for controlling annual weed with herbicides?
The best stage for controlling annual weeds with herbicides is usually the early growth stage. Controlling annual weeds with herbicides is most effective during their early growth stage, as they are more susceptible to the chemicals at this point in their development.
Applying herbicides during the early growth stage of annual weeds is most effective because they are smaller, more vulnerable, and less established.
This allows the herbicides to have maximum impact, inhibiting weed growth and preventing them from competing with desirable plants for resources.
Summary: Controlling annual weeds with herbicides is most effective during their early growth stage, as they are more susceptible to the chemicals at this point in their development.
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How many milliliters of concentrate sulfuric acid, which is 96% (w/w) pure H2SO4, are needed to prepare 500mL of a 2.0M solution of sulfuric acid? (molar mass = 98.08g/mol, density = 1.831g/mL)
a) 28 mL
b) 51 mL
c) 56 mL
d) 96 mL
Approximately 55.8 mL of 96% concentrated sulphuric acid is needed to prepare 500 mL of a 2.0 M solution of sulfuric acid.
To prepare 500 mL of a 2.0 M solution of sulphuric acid using 96% (w/w) concentrated sulfuric acid, follow these steps:
1. Calculate the moles of H2SO4 required for the 2.0 M solution:
Moles = Molarity × Volume
Moles = 2.0 mol/L × 0.5 L
Moles = 1.0 mol H2SO4
2. Convert moles to grams using the molar mass of H2SO4:
Mass = Moles × Molar mass
Mass = 1.0 mol × 98.08 g/mol
Mass = 98.08 g H2SO4
3. Calculate the mass of 96% concentrated sulphuric acid needed:
Mass of concentrated H2SO4 = (Mass of H2SO4) / (Percentage purity)
Mass of concentrated H2SO4 = 98.08 g / 0.96
Mass of concentrated H2SO4 = 102.17 g
4. Convert the mass of concentrated sulphuric acid to volume using the given density:
Volume = Mass / Density
Volume = 102.17 g / 1.831 g/mL
Volume ≈ 55.8 mL
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