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Pure HCl is 36.5 mwt so 0.5M would be 18.25 g pure HCl. In practice HCl is not pure but supplied at 36.5 % HCl typically.
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How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
Is oxycodone hcl m 05 52 the same as roxicodone 5 mg?
Yes m 0552 is generic roxycodone 5 mg
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 the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
Is oxycodone hcl m 05 52 the same as roxicodone 5 mg?
Yes m 0552 is generic roxycodone 5 mg
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 the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
Is 1 m HCl is more reactive than 4m HCl?
1 m HCl is not more reactive than 4m HCl, but 4m HCl is more concentrated.
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
What volume of 3.0 M HCl sould be obtained to prepare 100 mL of 1.0 M HCL?
33.3 ml of 3.0 M HCl should be filled up and mixed with water up to 100.0 ml of a 1.0 M HCl solution.
What is the molarity of an hcl solution if 7ml hcl solution is titrated with 27.6ml of 0.170m of naoh solution?
(7 mL)(X M HCl) = (27.6 mL)(0.170 M NaOH)7X = 4.692X = 0.7 M HCl==========
What is pH of 0.1 N HCL?
0.1 M HCl =============
How many ml of 6.00 M HCl are needed to prepare 1500 ml of 0.200 M HCl solution?
There is an easy way to calculate this, the formula is c1*V1= c2*V2 where c1 = stock concentration (in this case 8 M); c2 = wanted concentration ( 2 M); V1= how much volume of solution 1 (stock solution, in this case 8 M HCl) is needed; V2= desired volume of solution 2 (in this case 2 M HCl). To determine how much 8 M HCl you need you use a modification of the formula above. V1= (c2*V2 ) / c1 = (2 M * 0,150 l )/ 8 M = 0,0375 l So to make 150 ml 2 M hydrochloric acid you need to dissolve 37,5 ml of 8 M HCl in 112,5 ml H2O. Remember to always put acids into water and not the other way around!
How to prepare HCL solution?
Prepare HCl 1 M by HCl concentration 37 % HCl concentration 37 % have density =1.19 g/ml HCl 1 M use HCl 37 % 82.81 ml make volume with water to 1 liter
What calculation set-up would be correct to determine the volume of concentrated hydrochloric acid 12.0 M HCl that is required to make 500.0 milliliters of a 6.0 M HCl?
The answer is 19,67 mL HCl 6,1 M to obtain 1 L of HCl 0,12 M.
