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the division of no of solute in no of solution
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Why do solutions have different molarities?
The molarity of solution is the number of moles of solute per liter of solution. M (molarity ) = n / V = moles of solute / liters of solution = x.xxx M Thus, solutions can have different molarities because they can have different amounts of solute (in moles) per liter of solution.
How do you calculate average molarity?
From my understanding, it would be like any other average. You would take the the molarities of the solations, and add them up, and divide by the number of molarities. For example, let's say you did a titration using NaOH, and you did this 3 times, getting results like .30 M, .40 M, and .50 M, you would add those three up and get 1.2 M. Now you would divide that number by the number of titrations, which in this instance is obviously 3, so when you do that, you should get the average molarity of .40 M. Hope this helped at all. Bye.
How many millilieters of 5.5 m naoh are needed to prepare 300 ml of 1.2 m naoh?
Use M1V1=M2V2 Where M is the concentration (5.5 m for M1 and 1.2 m for M2) and V is volume V1 is 300 ml and V2 is your unknown. Using this calculation for other questions be sure that units are all the same. So all molarities and all mL in this example.
The salt formed during the reaction between pottassium hydroxide and hydrochloric acid is?
The reaction between Potassium Hydroxide and Hydrochloric Acid is a simple double-replacement reaction. (Remember to memorize your polyatomic ions and reaction rules! It comes in handy)KOH + HCl --> KCl + H2OHydroxides are always strong bases and hydrochloric acid is one of the strongest acids (especially at high molalities or molarities [pH differs according to acid/base concentration]). When a base reacts with an acid, a salt and water ALWAYS forms. This is called a neutralization.
What mass of calcium carbonate in grams can be dissolved by 3.9g of HCl?
To solve this, you have to be aware that this is a acid-base reaction, and that HCl is a gas, that usually is not applied in this form.However: Hydrochloric acid reacts with the calcium salt of carbonic acid, to form calcium chloride, water and (volatile) carbon dioxide.Thus, you must first calculate the moles (n) of H+ contained in 3.9g of HCl. 1 mole of HCl contains 1 mole of H+. So you can calculate:M(HCl) = M(H) + M(Cl) = 36.45g/molm(HCl) = 3.90gn(HCl) = m(HCl) / M(HCl) = 0.11molNext, you must calculate the moles of carbonate that can be dissolved.Using the following formula:CO32- + 2 H+ ↔ H2O + CO2↑you can see, that you need 2 moles of H+ for 1 mole of CO32-.Subsequently, you have to calculate the molar mass of calcium carbonate:M(CaCO3) = 40.08g/mol + 12.01g/mol + 3*16.00g/mol = 100.09g/molAnd finally, you can calculate the mass of calcium carbonate you can dissolve using 0.11mol HCL:m(CaCO3)= M(CaCO3) * [½ * n(HCl)] = 5.35gFrom the equations above, considering the molarities, we can draw a more dense formula that allows us to neglect the absolute molarities, so we only have to use the relative molarities. The equation can also be used to check if we calculated correctly)m(A)/(2*M(A)) = m(B)/M(B)We transpose to calculate m(B):m(B)= (½*m(A)/M(A))*M(B)and when we insert the values:m(CaCO3) = (0.50*(3.90g/36.45g/mol))*100.09g/mol = 5.35gAnd next time, you'll be able to do this by yourself ;)
Why do solutions have different molarities?
The molarity of solution is the number of moles of solute per liter of solution. M (molarity ) = n / V = moles of solute / liters of solution = x.xxx M Thus, solutions can have different molarities because they can have different amounts of solute (in moles) per liter of solution.
How do you calculate average molarity?
From my understanding, it would be like any other average. You would take the the molarities of the solations, and add them up, and divide by the number of molarities. For example, let's say you did a titration using NaOH, and you did this 3 times, getting results like .30 M, .40 M, and .50 M, you would add those three up and get 1.2 M. Now you would divide that number by the number of titrations, which in this instance is obviously 3, so when you do that, you should get the average molarity of .40 M. Hope this helped at all. Bye.
The Atlantic pacific and Caribbean are oceans with concentrations of 0.438 m licl and 0.0512 m mgcl2 what are the molarities what ions in solution a c and the total ion concentration d?
Hi its me again;} I dont really know this one but if you goole search it you would get it.Even dough I am in the 8 grade I still don't know this!
How many millilieters of 5.5 m naoh are needed to prepare 300 ml of 1.2 m naoh?
Use M1V1=M2V2 Where M is the concentration (5.5 m for M1 and 1.2 m for M2) and V is volume V1 is 300 ml and V2 is your unknown. Using this calculation for other questions be sure that units are all the same. So all molarities and all mL in this example.
The salt formed during the reaction between pottassium hydroxide and hydrochloric acid is?
The reaction between Potassium Hydroxide and Hydrochloric Acid is a simple double-replacement reaction. (Remember to memorize your polyatomic ions and reaction rules! It comes in handy)KOH + HCl --> KCl + H2OHydroxides are always strong bases and hydrochloric acid is one of the strongest acids (especially at high molalities or molarities [pH differs according to acid/base concentration]). When a base reacts with an acid, a salt and water ALWAYS forms. This is called a neutralization.
What mass of calcium carbonate in grams can be dissolved by 3.9g of HCl?
To solve this, you have to be aware that this is a acid-base reaction, and that HCl is a gas, that usually is not applied in this form.However: Hydrochloric acid reacts with the calcium salt of carbonic acid, to form calcium chloride, water and (volatile) carbon dioxide.Thus, you must first calculate the moles (n) of H+ contained in 3.9g of HCl. 1 mole of HCl contains 1 mole of H+. So you can calculate:M(HCl) = M(H) + M(Cl) = 36.45g/molm(HCl) = 3.90gn(HCl) = m(HCl) / M(HCl) = 0.11molNext, you must calculate the moles of carbonate that can be dissolved.Using the following formula:CO32- + 2 H+ ↔ H2O + CO2↑you can see, that you need 2 moles of H+ for 1 mole of CO32-.Subsequently, you have to calculate the molar mass of calcium carbonate:M(CaCO3) = 40.08g/mol + 12.01g/mol + 3*16.00g/mol = 100.09g/molAnd finally, you can calculate the mass of calcium carbonate you can dissolve using 0.11mol HCL:m(CaCO3)= M(CaCO3) * [½ * n(HCl)] = 5.35gFrom the equations above, considering the molarities, we can draw a more dense formula that allows us to neglect the absolute molarities, so we only have to use the relative molarities. The equation can also be used to check if we calculated correctly)m(A)/(2*M(A)) = m(B)/M(B)We transpose to calculate m(B):m(B)= (½*m(A)/M(A))*M(B)and when we insert the values:m(CaCO3) = (0.50*(3.90g/36.45g/mol))*100.09g/mol = 5.35gAnd next time, you'll be able to do this by yourself ;)
What is an example of a concentrated solution?
Drinking squash, concentrated vegetable boullion (stock), some fruit juices are concentrated then diluted again... basically anything that has been boiled to remove the water content is "concentrated".
What is buffer capacity and what are the factors that effect the buffer capacity?
it is defined the capability of a buffer to resist the change of pH.it can be measured quantity that how much extra acid or base , the solution can absorb before the buffer is essentially destroyed. buffer capacity of a buffer solution is determined by the sizes of actual molarities . so , a chemist must decide before making the buffer solution.
How is a particulate formed?
I will assume you are asking about the formation of an ionic compound when two solutions come together. Ions attract at a site of nucleation. All compounds are soluble to some extent (sometimes to a very, very limited extent). We describe this mathematically by the division: ([product 1]*[product 2]) ÷ ([reactant 1]*[reactant 2]) = Ksp (for a perfectly saturated solution) If the molarities of the actual solution in question exceed Ksp when this calculation is performed, we predict that precipitate will form. We may encourage particle growth in a number of ways. You can raise the temperature to decrease the chance of supersaturation. More energy per particle leads to formation of the colloid. You can mix the species slowly, by either physical or chemical means. This prevents local supersaturation. You can keep your solutions dilute. This prevents the particles from becoming so small they would pass through a filter. You can add a soluble background electrolyte. An ionic environment will encourage particles to come together.
How would you prepare dilute sulfuric acid from concentrated sulfuric acid for use in an experiment?
Add the acid to water. Do NOT add water to the acid as it will boil and split acid everywhere. Please say 100 mL of water in a beaker and slowly add sulphuric acid to it. To change the molarities of the acid you need to do come calculations. If you have say 50mL of 5M sulphurtic acid and you want to make it say 1M sulphuric acid. Then use the eq'n moles = [conc] X vol(mL) / 1000 So 5M x 50mL / 1000 = 1M x vol(mL)/1000 Algebraically rearrange/. vol(mL) = 5M x 50mL / 1M NB THe '1000' cancel down. vol(mL) = 250mL In this case have 175 mL of water in a beaker, slowly add the 50mL (H2SO4), to avoid spitting. You will then have 225 mL. So then slowly add a further 25 mL of water to make the concentration 1M. NB 225mL of sol'n will be of the wrong concentration, that is why you add a small final amount of water.
If two solutions having different osmolarities are separated by a water-permeable membrane will there be a change in the volume of the two compartments if the membrane is impermeable to solutes?
Water will flow from a region of higher concentration to lower concentration until the two osmolarities are equal if the membrane is impermeable to the solute. A change in the volume of the solution would be the result. If it is permeable then the solute will diffuse simultaneously from the higher solution to the lower solution until equilibrium is reached. The volume will not change in this case.
Can a solution be isosmotic but not isotonic?
Reasons and explanation -Isotonic solutions contain only non-penetrating solutesand have the same osmotic pressure as the cells they surround. They are neither absorbed nor do they absorb anything from the surrounding cell. They have the same concentration of salt as the blood and human cells in the body.whereasIsosmotic solutions contain both penetrating and non-penetrating solutes. They have the same osmotic pressure of the surrounding cells. Penetrating solutes are solutes that can pass through the membrane of the cell and increase the osmotic pressure in the cell. This forces the cell to absorb more water to equalize the difference in pressure. This may lead to bursting of the cell when too much water is absorbed.
