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What volume of a 0.5 M solution can be made using 0.79 moles of Ca(OH)2?
Kayonna Cobbin
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750 ml of 20M HCl is mixed with 250 ml of 60M HCl What is the new molarity?
Molarity of a solution is the number of moles of the solute divided by the volume of the solution (in liters). If 750 ml of 20M HCl is mixed with 250 ml of 60M HCl, we first find the total number of moles of HCl in our new solution. Using that same formula, M=moles/V, we cansee that moles=MV. In the first solution we have (20M)(0.750L) = 15 moles. In the second, (60M)(0.250L) = 15 moles, so we have a total of 30 moles in our new solution, which also has a volume of 750mL + 250mL = 1L. The molarity of the new solution is 30 moles/1L = 30M
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
Can Draw a sketch of devices using to find-out the volume of liquids?
Volume (cm3) = (Number of Moles X 1000) Divided by Concentration Volume (dm3) = Number of Moles Divided by Concentration
How many grams of NaOH are contained in 500mL of 0.5M NaOH?
First, you must find the amount of moles of NaOH, using the concentration and volume given. By lowercase m, I'm assuming you mean molality, or molals of solution, which is the equation:molality (m) = (moles of solute) / (total volume of solution (in liters))To solve for moles of NaOH, your solute, rearrange the equation by multiplying volume on both sides to get:moles solute = (molality)(total volume of solution)Next, just plug in the information you know, which is 500 mL for the total volume and 125 m for the molality.***Volume for concentration problems must be converted to liters, so remember that 1 L = 1000 mLmoles NaOH = (125 m)(0.500 L) = 62.5 molesFinally, convert this to grams by finding the molar mass of NaOH using the periodic table:22.99 + 16.00 + 1.008 = 39.998 g/mol62.5 moles (39.998 g) / (1 mol) =249.875 grams NaOH
How does would you make 1 liter out of 2 moles?
By using a 2Molar solution.
How much space will 2.3 grams of sulfur dioxide take up at standard temperature and pressure?
we first find the number of moles( number of moles= mass/molar mass). the we can find the volume by using the formule( volume=number of moles multiplyd by the molar volume)
How can you prepare a dilute solution?
Before reading this answer, I recommend that you look at the question under the Related Questions links to the left of this answer "How do you prepare a solution of a specific concentration by dissolving a solid in a liquid?"You must know two things to make a solution: the number of moles of the solute, and the number of liters of solution. Then you will add the correct volume of the concentrated solution so that you have the right number of moles, and then add water until the total volume is correct.To make a solution from another solution by diluting it, you first need to know how many moles of solute you need in the final solution. That's very easy! You need to know the concentration of the final solution and its volume. Then just multiply those two together to get the number of moles of solute you need:Equation 1) Moles of solute = Molarity * liters of solutionNow you know how many moles you need, you just have to figure out how to them them! To do that, we'll use the same equation, but now rearranged in a different order. We want to know how many liters of the original (concentrated) solution we need to get the correct number of moles. So just dividing both side by "Molarity" we get:Equation 2) Liters of Solution = Moles of solution ÷ MolaritySo that will tell us how much concentrated solution to use. Then just add that much of the concentrated solution to enough water so that the total volume is correct.-- Step #1: Determine the concentration and total volume of the new solution you want to make (probably given to you in the question you are solving!)-- Step #2: Determine how many moles of solute must be present in that solution, using Equation 1-- Step #3: Determine what volume you need (how many liters) of the concentrated solution you need to get the number of moles you got in Step #2, now using Equation 2-- Step #4: Add the volume of concentrated solution you determined in Step #3 to the correct amount of water so that the total volume is what you need (from Step #1). HOWEVER, WHEN DILUTING A STRONG ACID, ALWAYS ADD ACID TO WATER! SAME FOR A STRONG BASE! To do this, just estimate how much water you will need to add (the total volume minus the volume from Step #3), and add a little less than this. Then add the concentrated acid to that, and then add a bit more water to get the exact volume correct.-- Let me do a couple of examples now:--Example 1: How do you make 200 mL of a 0.1 M solution of hydrochloric acid (HCl) from a solution of 1.0 M HCl?--Answer: First let's find how many moles of HCl we need in our diluted solution. Using Equation 1, we have:Moles of HCl = 0.2 L * 0.1 M = 0.02 moles(remember that 200 mL = 0.2 L)Now how many liters of the 1.0 M solution do we need to get 0.02 moles? Now using Equation 2:Volume of 1.0 M solution = 0.02 moles ÷ 1.0 M = 0.02 LAnd again, 0.02 L is equal to 20 mLSo to make our solution, we are going to ADD ACID TO WATER. So, first add about 150 mL of water to a flask. Then add 20.0 mL of 1.0 M HCl. Then add as much water as necessary to that the total volume is exactly 200 mL. This is usually done in what is called a volumetric flask -- and you'd want to use a 200 mL volumetric flask in this case.--- Example 2: How do you make 2.0 liters of a 0.231 M solution of potassium nitrate (KNO3) from a 3.0 M solution of KNO3?--- Answer: Same as before, how many moles of KNO3 do we need in the diluted solution?Moles of KNO3 = 0.231 M * 2.0 L = 0.462 moles.Now how many liters of 3.0 M solution do we need to get that many moles?Liters of 3.0 M solution = 0.462 moles ÷ 3.0 M = .154 LAnd again, that 154 mL.To make our solution, we will add 154 mL of the 3.0 M KNO3 solution to a volumetric flask, and then add as much water as we need so that the total volume is exactly 2.0 liters (use a 2 liter volumetric flask for this!)
What is the molarity of the following solution 1.0 moles of KCl in 500mL of solution?
You need to bring this to a litre. If there is 1 mole in 500ml (using ratio), there will be 2 moles in a litre. So your molarity is 2.
What the formula for molarity?
Molarity is the number of moles of solute dissolved in one liter of solution. The units of molarity are moles per litre iemoles of solute per litre of solution. The equation for molarity is: (moles of solute)/(litres of solution) Eg 3 moles per litre or 3 mol L-1 Alternatively, volume can be measured in cubic decimeters: dm3 which are equal to litres. Eg 3 moles dm-3 is the same as 3 mol L-1 See:http://dl.clackamas.edu/ch105-04/molarity.htm
Estimation of the amount of Zn present in the given solution of ZnCl2 using 0.01M EDTA solution.?
The amount of zinc is 0,01 moles.
How can you convert moles to liters?
First of all, you have to know what substance you are dealing with. Then you would have to know its density. Using the density you can convert liters to kilograms. Then you get the gram-molecular weight (using the chemical formula of this substance and the Periodic Table of Elements) and with that you can convert kilograms to moles.
An aqueous KNO3 solution is made using 89.9g of KNO3 diluted to a total solution volume of 1.35L?
1.0 molal
