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Calculate the final concentration (in Molarity) when 25 mL of water is added to 95 mL of 1.4 M LiCl.?
Wiki User
∙ 7y ago
25 ml added to 95 ml give a final volume of 120 ml (95 ml)(1.4 M) = (120 ml)(x M)
x = 1.1 M
Wiki User
∙ 7y ago
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If 20.00mL of a 1.50M solution of KBr is diluted to a final volume of 150.0mL what is the new molar concentration?
initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
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 final percent concentration of the solution when 600 ml of 100 percent methanol added to 4400 ml of water?
13.6% methanol solution.
What is the molarity of a solution that is made using 1.2 moles of a substance in 500mL?
Molarity (M) is defined as moles of solute/liters of solution. Assuming the final volume is 500 ml (0.5 liters), then M = 1.2 moles/0.5 liters = 2.4 M
What is 4 ml of chemical added to 1liter of water in many ppm concentration?
4ml/1000 = approx 4000 ppm, depending on the final volume after adding 4ml to 1000 ml water
How do you calculate the concentration of two mixed solutions?
calculate final molarity of the solution if 11ml of 5m solution is made up to 20ml
If 20.00mL of a 1.50M solution of KBr is diluted to a final volume of 150.0mL what is the new molar concentration?
initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
What is the effect on the molarity of a solution of adding more solvent to a solution?
Adding more solvent to a solution decreases the molarity of the solution. This is based on the principle that initial volume times initial molarity must be equivalent to final volume times final molarity.
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 final molarity of 5.84 grams of Na Cl?
Depending on the volume of water ! For 1 L, the molarity is approx. 0,1.
When 200 mL of water are added to 100mL of 12 percent KCL solution the final concentration of KCL is?
4.0%
What is the final percent concentration of the solution when 600 ml of 100 percent methanol added to 4400 ml of water?
13.6% methanol solution.
What is the molarity of a solution that is made using 1.2 moles of a substance in 500mL?
Molarity (M) is defined as moles of solute/liters of solution. Assuming the final volume is 500 ml (0.5 liters), then M = 1.2 moles/0.5 liters = 2.4 M
What is 4 ml of chemical added to 1liter of water in many ppm concentration?
4ml/1000 = approx 4000 ppm, depending on the final volume after adding 4ml to 1000 ml water
What is the concentration of a solution prepared by diluting 20.0mL of a 0.200 M NaCl to 250.0 mL?
Use the equation M(initial)*V(initial)=M(final)*V(final). In this case, M(initial) is 0.200 M NaCl. V(initial) is 20.0mL. V(final) is 250.0mL. You are solving for M(final). To solve, you rearrange the equation so M(final)=(M(initial)*V(initial))/V(final), which gives you (0.200*20.0)/250. The answer is 0.016 M for M(final). You don't need to convert mL to L in this type of problem. You can if you want, but you will end up with the same answer. It's just an extra unnecessary step, unless the question is asking for a Volume in L. But in this case you were asked for concentration (Molarity), so no volume conversions were necessary.
What is the molarity of 6 moles of NaCl dissolves in 2 L of water?
Molarity is defined as moles solute/liter of solution6 moles/2 liters solution = 3 molar NOTE: This assumes no volume change and 2L is the final volume of solution.
What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?
We must first figure out the amount of NaCl in moles: M = mol/L = mmol/mL 6 = mmol/25 mL 150 mmol NaCl Now divide by the total volume to get the final concentration: 150 mmol/100 mL = 1.5 M NaCl
