The strength of an acid is the extent to which it is dissociated into ions in dilute solution, and cannot be calculated from a molarity, which is a measure of concentration, not strength. Hydrocholoric acid is a strong acid. It is completely dissociated in I M solution.
1.46 m 100cm = 1 m
The equation to calculate the work done is: Work done (J) = force applied (n) x distance moved of force (m)
A search on Google for "1 meter in feet" gives 3.2808399 feet.Direct Conversion Formula 1 m*1 ft0.3048 m=3.280839895 ft
82.02 ft 1 m = 3.28 ft 1 ft = 0.3048 m
The sort of question that demonstrates why the metric system is easier to calculate with! The easy bit: 1 m = 100 cm 32 m - 3200 cm The harder bit: 1 yard = 3' 1' = 12" 1" = 2.54 cm Work all that through, and we can see that 3200 cm (32 m) is 1259.843". Which is 104.987'. Which is 34.996 yards, i.e. about 1/6" short of 35 yards.
1 m HCl is not more reactive than 4m HCl, but 4m HCl is more concentrated.
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.
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
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 ;)
percentage = well, mostly weight percentage is the most commonly given percentage density = the density of a sol'n is constant, for HCl, the value is 1.18 g/ mL now assuming you have 34% of HCl in the sol'n in preparing 1M HCl, calculate the mass of HCl Needed. assuming there are 100g of the whole solution, therefore there will be 34g of HCl: percent by weight = (34% x 100g) / 100g = 34g now to get the mass, we need dimensional analysis. 34 g HCl x 1 mol HCl x 1 L sol'n x 1.18 g HCl x 1 mL = FINAL ANSWER 36.45 g HCl 1 mol HCl 1 mL 1 L sol'n you just get the final answer.... percentage = well, mostly weight percentage is the most commonly given percentage density = the density of a sol'n is constant, for HCl, the value is 1.18 g/ mL now assuming you have 34% of HCl in the sol'n in preparing 1M HCl, calculate the mass of HCl Needed. assuming there are 100g of the whole solution, therefore there will be 34g of HCl: percent by weight = (34% x 100g) / 100g = 34g now to get the mass, we need dimensional analysis. 34 g HCl x 1 mol HCl x 1 L sol'n x 1.18 g HCl x 1 mL = FINAL ANSWER 36.45 g HCl 1 mol HCl 1 mL 1 L sol'n you just get the final answer....
.260 M of HCL, not 260 More than likely correct, but, - log(0.260 M HCl) = 0.6 pH ----------- ( pH can be below 1 )
According to I.P. 1996
The answer is 19,67 mL HCl 6,1 M to obtain 1 L of HCl 0,12 M.
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
Find moles HCl. 5 g HCl (1 mole HCl/36.450 grams) = 0.1372 moles HCl Now, Molarity = moles of solute/Liters of solution Molarity = 0.1372 moles HCl/1 liter = 0.1372 M HCl Then. -log(0.1372 M HCl) = 0.9 pH ( you might call it 1, but pH can be off the scale ) -----------
37% HCL equals to 12.18 M. So you can caculate 32% is 10.53 M. That means for preparing 1 L 1.5 M HCL, you need mix 142.45 mL 32% with 857.55 mL dH2O.
It doesn't matter how much you have, HCl (Hydrochloric Acid) has a pH of 1