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What is the molarity of a solution with 0.2 moles of KOH in 100 mL of water?
Molarity = moles of solute/Liters of solution get moles KOH 6.31 grams KOH (1 mole KOH/56.108 grams) = 0.11246 moles KOH 0.250 M KOH = 0.11246 moles KOH/XL 0.11246/0.250 = 0.4498 liters = 450 milliliters
What is the pH of a solution prepared by dissolving 0.140 g KOH in sufficient water to prepare 250.0 ml of solution?
Okay to calculate this, you must first calculate the number of moles KOH forms in water. This is simply done by dividing mass by the molecular mass. Therefore: 0.140 / (19+16+1) Then, you need to know how KOH dissociates in water, which is luckily 1:1. Therefore, the number of moles of OH is also 0.140 / (19+16+1). Then you find the concentration of OH, which is number of moles divided by the volume (do it in litres): (0.140 / (19+16+1))/0.25 Then, you find the pOH. This would be -log ((0.140 / (19+16+1))/0.25) Then, you get this answer and minus if from 14: 14-(-log ((0.140 / (19+16+1))/0.25)) Make sure you actually do these steps as remember every problem is different so you need to know the process, not the answer.
What is the pH KCl?
1. Identify (a) through (d) as reactants or products. Type your answers in the spaces provided: (a) (b) (c) (d) KOH + HCl KCl + H2O
What is the concentration of an HBr solution if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
The reaction between HBr and KOH is a 1:1 ratio. This means that the moles of HBr present in the solution will be equal to the moles of KOH used in the neutralization reaction. Using this information and the volume and concentration of KOH used, you can calculate the concentration of the HBr solution.
How does a solution with a pH of 2 compare to a solution with a pH of 1?
A solution with a pH of 2 is less acidic than a solution with a pH of 1. The pH scale is logarithmic, so each unit change represents a tenfold difference in acidity. Therefore, a solution with a pH of 1 is 10 times more acidic than a solution with a pH of 2.
What is the molarity of a solution with 0.2 moles of KOH in 100 mL of water?
Molarity = moles of solute/Liters of solution get moles KOH 6.31 grams KOH (1 mole KOH/56.108 grams) = 0.11246 moles KOH 0.250 M KOH = 0.11246 moles KOH/XL 0.11246/0.250 = 0.4498 liters = 450 milliliters
What solution has a greater concentration of hydrogen ions a solution with a pH of 3 of a pH of 5 Explain?
1/103 = 0.001 M ========( pH 3 ) 1/105 = 0.00001 M ============( pH 5 ) As you see, a pH of 3 has a 100 times concentration of 5 pH ( 10 * 10 devalued ) This is the scale; logarithmic.
What is the pH of a solution prepared by dissolving 0.140 g KOH in sufficient water to prepare 250.0 ml of solution?
Okay to calculate this, you must first calculate the number of moles KOH forms in water. This is simply done by dividing mass by the molecular mass. Therefore: 0.140 / (19+16+1) Then, you need to know how KOH dissociates in water, which is luckily 1:1. Therefore, the number of moles of OH is also 0.140 / (19+16+1). Then you find the concentration of OH, which is number of moles divided by the volume (do it in litres): (0.140 / (19+16+1))/0.25 Then, you find the pOH. This would be -log ((0.140 / (19+16+1))/0.25) Then, you get this answer and minus if from 14: 14-(-log ((0.140 / (19+16+1))/0.25)) Make sure you actually do these steps as remember every problem is different so you need to know the process, not the answer.
What is the molarity of a solution when 50.0ml of a 4.00M KOH solution is diluted to 200ml. what is the percent concentration of KOH in this final solution. asume the density of 1.0gmole?
The concentration is 1 mol/L or 5,611 g KOH/100 mL solution.
What is the concentration of an HBr solution if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
The reaction between HBr and KOH is a 1:1 ratio. This means that the moles of HBr present in the solution will be equal to the moles of KOH used in the neutralization reaction. Using this information and the volume and concentration of KOH used, you can calculate the concentration of the HBr solution.
What is the pH KCl?
1. Identify (a) through (d) as reactants or products. Type your answers in the spaces provided: (a) (b) (c) (d) KOH + HCl KCl + H2O
How does a solution with a pH of 2 compare to a solution with a pH of 1?
A solution with a pH of 2 is less acidic than a solution with a pH of 1. The pH scale is logarithmic, so each unit change represents a tenfold difference in acidity. Therefore, a solution with a pH of 1 is 10 times more acidic than a solution with a pH of 2.
How do you make a 1 percent aqueous solution of potassium hydroxide?
To make a 1% aqueous solution of potassium hydroxide, you would mix 1 gram of potassium hydroxide with 99 grams of water (for a total of 100 grams solution). This would give you a solution where 1% of the total weight is potassium hydroxide.
What is the molarity of a KOH solution if 24.6 mL neutralizes 44.0 mL of a 0.211 M HCl?
To find the molarity of the KOH solution, we first need to determine the number of moles of HCl used in the reaction (n(HCl) = Molarity x Volume). Then, since KOH and HCl react in a 1:1 ratio, the number of moles of KOH will be the same. Finally, calculate the molarity of KOH using the moles of KOH and the volume of KOH solution used.
How many times a solution of pH 1 will be stronger than that of a solution having pH 2?
A solution with pH 1 is 10 times stronger (more acidic) than a solution with pH 2. This is because pH is measured on a logarithmic scale, with each unit representing a tenfold difference in concentration of hydrogen ions.
Is a solution with a pH of 2 twice or half as acidic as a pH of 1?
A solution with a pH of 2 is ten times less acidic than a solution with a pH of 1, not half as acidic. pH is a logarithmic scale, so each unit change represents a tenfold difference in the concentration of hydrogen ions.
How many times more acidic is a solution of pH 1 than a solution having pH 2?
To first answer this question you must know how the PH scale works. Essentially the PH scale is a logarithmic scale. A logarithmic scale unlike a linear scale (you know the scales that go from 1, 2, 3, etc.) works using exponential increments. For the PH scale every time you go one number down the solution the item in question becomes ten times more acidic than the number above. Therefore to ultimately answer your question a solution with a PH of 1 is ten times more acidic than a solution that has a PH of 2.
