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A solution containing what pairs of substances will be a buffer solution?
A) NaI, HI B) KBr,HBr C) RbCl, HCl D) CsF, HF
What is a saurated solution?
when the solute can no longer dissolve in a solution then the solution can be said as saturated
How does a graph show a saturated solution and a unsaturated solution?
A graph can illustrate what solution is saturated and unsaturated. If the point is on the line, then the solution is saturated, while if is below the line, the solution is unsaturated.
If a seed crystal was added to a supersaturated solution how would you characterize the resulting solution?
If a seed crystal was added to a supersaturated solution, the resulting solution would be a crystallized solution. The formation of solid crystals that precipitate from a solution is called crystallization.
What solution with a low concentration of solute?
A dilute solution.
How can prepare .01N KBr solution?
To prepare a 0.01N KBr solution, dissolve 0.74g of KBr in 1 liter of water. This will give you a solution with a molarity of 0.01N for KBr.
How many moles of kbr are present in 25ml of a 1.5 M solution?
To find the number of moles of KBr in the solution, first calculate the number of moles of KBr in the 25 mL solution using the given concentration and volume. $$moles = concentration \times volume$$ Then, multiply the moles by the molecular weight of KBr to get the mass of KBr in the solution if needed.
If you have 670.0 grams of water and wish to make a 2.13 m solution of KBr how many grams of the solute would you have to add to the water that you have?
To make a 2.13 M solution of KBr, you need to determine the number of moles of KBr required using the formula Molarity = moles of solute / volume of solution in liters, then calculate the mass of KBr needed using its molar mass. Once you have the mass of KBr, you can add it to the water to prepare the solution.
Is KBr soluble?
Yes, potassium bromide (KBr) is soluble in water. It forms a clear, colorless solution when dissolved.
What is the mole of the concentration of KBr in a solution prepared by dissolving 2.21g of KBr in 897g of water?
The answer is 0,0207 mol.
How many grams of KBr are present in 300.0 mL of a 1.25 M solution?
To find the grams of KBr in the solution, first calculate the moles of KBr present by using the molarity formula: moles = Molarity x Volume (L). Then, convert moles of KBr to grams using its molar mass. For KBr, the molar mass is approximately 119 g/mol. Finally, perform the calculation to find the grams present in the solution.
How many moles of KBr are present in 190mL of a 0.265M solution?
The answer is 0,0509 mole.
How many moles of KBr are present in 110mL of a 0.290M solution?
To find the number of moles of KBr in the solution, first convert the volume to liters (110mL = 0.110L). Then, use the formula: moles = molarity x volume in liters. So, moles of KBr = 0.290 mol/L x 0.110 L = 0.032 moles of KBr.
Which solution would elevate the boiling point of water the most MgF2 glucose KNO3 KBr?
MgF2
How many grams of solute are present in 365 mL of 0.590 M KBr?
To find the grams of solute, first calculate the moles of KBr in 365 mL of 0.590 M solution. This is done by multiplying the volume (in liters) by the molarity. Then, use the molar mass of KBr to convert moles to grams.
How many moles of kbr are in 68.5 ml of a 1.65m solution?
To find the number of moles of KBr in a 1.65 M solution, you can use the formula: [ \text{moles} = \text{molarity} \times \text{volume (L)} ] First, convert 68.5 mL to liters: 68.5 mL = 0.0685 L. Then, multiply by the molarity: [ \text{moles} = 1.65 , \text{mol/L} \times 0.0685 , \text{L} \approx 0.113 , \text{moles} ] So, there are approximately 0.113 moles of KBr in 68.5 mL of a 1.65 M solution.
KBr a strong or weak base?
KBr is not a base, but a salt formed by the combination of the strong base KOH and the strong acid HBr. It is considered a neutral salt since it does not significantly contribute to the pH of a solution.
