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Assuming the Ka= [H+][PO2-]/[PO3-] and that PO3=PO2- then we can safely assume Ka= [H+][PO2-]/[PO2-] and so Ka= [H+][PO2-]/[PO2-] Ka=[H+] since the Ka of Phosphoric acid is equal to 7.5x10-3 then we can take -log(7.5x10-3) to find the pH=2.12
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What is h2po4 in chemistry?
H2PO4- is called dihydrogen phosphate ion. It is the conjugate base of Phosphoric Acid H3PO4 and the conjugate acid of monohydrogen phosphate ion HPO42-Liquid
What is the conjugate base for HPO3 -2?
H3PO4 (aq) + H2O (l) ---> 2H3O+ (aq) + PO4-3 (aq)donor acid + acceptor base ---> conjugate acid + conjugate basethe answer above is wrongto form a conjugate, the ion H2PO4 - must lose a hydrogen ion H+i.eH2PO4 - -H+ = HPO4 2-(conjugate base)
How many moles of O2 are in one mole of H3PO4?
Actually H3PO4 is a molecular formula referring to the compound we know as Phosphoric acid. It doesn't indicate number of moles of H3PO4. But the number of moles can be found out if the amount in mass or some other measurable quantity(e.g. conc. in solution) is given. The molar mass(mass of 1 mole) of H3PO4 is 98 grams. So if mass is given then it can be converted to grams and dividing by molar mass(i.e 98) we get number of moles. moles of H3PO4 =(mass of H3PO4 in grams)/98. 1 mole of H3PO4 has ->3 moles of H atoms. ->1 mole of P atoms. ->4 moles of O atoms. ( 1 mole=6.0225 *1023 units)
What mass of each product results if 750 mL of 6.00 M H3PO4 reacts to the equation?
What I would first is to find the amount of mols of H3PO4. Since you know that 1 M means there is 1 mol of solution in every 1 liter, you can figure out the moles of the solution. The solution is 6M, so that means that to find the moles of solute in the solution you multiply .750 (750 milliliters converted to liters) by 6. I think you did something similar, but .0075 L makes 7.5 milliliters. This will give you 4.5 mols of H3PO4.Now you can use stoichiometry to find the grams of Ca3(PO4)2. The balanced equation states that it takes 2 mols of H3PO4 to get 1 mol of Ca3(PO4)2:4.5 mol H3PO4 * 1 mol Ca3(PO4)2 / 2 mol H3PO4 = 2.25 mol Ca3(PO4)2Find the molar mass of Ca3(PO4)2 to convert the mols to grams:3*40 + 2*31 + 8*16 = 310 grams / mol2.25 mol Ca3(PO4)2 * 310 grams Ca3(PO4)2 / 1 mol Ca3(PO4)2 = 697.5 grams Ca3(PO4)2You can use the same process to find the mass of water.4.5 mol H3PO4 * 6 mol H2O / 2 mol H3PO4 = 13.5 mol H2O13.5 mol H2O * 18 g H2O / 1 mol H2O = 243 g H2OHope that helped! NB this is not my work just saw it on another website
What is the sequence of events that would occur when acid is added to phosphate buffer.?
There are different variations of phosphate buffer, but if we take the one in which NaH2PO4 is in equilibrium with Na2HPO4, then we can write the following:H2PO4^- H+ + HPO4^2-When and acid (H+) is added, it will react with HPO4^2- to produce H2PO4^-. Since H2PO4 is a weak acid, it will not dissociate appreciable, thus effectively removing the added H+ from solution and maintaining the pH.
What is h2po4 in chemistry?
H2PO4- is called dihydrogen phosphate ion. It is the conjugate base of Phosphoric Acid H3PO4 and the conjugate acid of monohydrogen phosphate ion HPO42-Liquid
What is the conjugate base for HPO3 -2?
H3PO4 (aq) + H2O (l) ---> 2H3O+ (aq) + PO4-3 (aq)donor acid + acceptor base ---> conjugate acid + conjugate basethe answer above is wrongto form a conjugate, the ion H2PO4 - must lose a hydrogen ion H+i.eH2PO4 - -H+ = HPO4 2-(conjugate base)
How do prepare phosphate buffer pH 4.5?
There is NO good buffer with phosphate for pH = 4.5, because pKa-value's differ too much from 4.5: pKa = 2.13 and 7.21 for H3PO4 and H2PO4- respectively.A good alternative would be Acetic acid / Acetate in molar ratio of about 2 : 1, because pK(acetic acid) = 4.77 .More precisely you can use the formula, based on the Henderson-Hasselbalch equation:log[acid]/[conjug.base] = = 4.77 - 4.5 = 0.27or[acid]/[conjug.base] = 10(pKacid -pHbuffer) = 100.27 = inv.log(0.27) = 1.82Doing the same for a H3PO4 / H2PO4- buffer, this results in[H3PO4/H2PO4-] = 10(pKacid -pHbuffer) = 10(2.13-4.5) = inv.log(-2.37) = 4.3*10-3or for H2PO4-/HPO42- buffer, this results in [H2PO4-/HPO42-] = 10(7.21-4.5) = 102.71 = inv.log(2.71) = 5.1*102Both ratio's are far beyond values for optimal buffercapacities: 0.1 < ratio < 10
How many moles of O2 are in one mole of H3PO4?
Actually H3PO4 is a molecular formula referring to the compound we know as Phosphoric acid. It doesn't indicate number of moles of H3PO4. But the number of moles can be found out if the amount in mass or some other measurable quantity(e.g. conc. in solution) is given. The molar mass(mass of 1 mole) of H3PO4 is 98 grams. So if mass is given then it can be converted to grams and dividing by molar mass(i.e 98) we get number of moles. moles of H3PO4 =(mass of H3PO4 in grams)/98. 1 mole of H3PO4 has ->3 moles of H atoms. ->1 mole of P atoms. ->4 moles of O atoms. ( 1 mole=6.0225 *1023 units)
What would NH4I plus H2O equals?
Ammonium Iodide solution.
What is the solution to 56 equals x - 7?
49
How would you find a solution to y equals 3x-5x?
8
What type of reaction is h3po4 plus 3koh equals k3po plus 3h2o?
Your reaction is this...H3PO4 + 3KOH --> K3PO4 + 3H2OThis type of reaction is called a double replacement.Note: You didn't put a 4 on the oxygen on the phosphate group on the product side in your question. If it wasnt there the equation would not have been balanced so i put it in myself.
What mass of each product results if 750 mL of 6.00 M H3PO4 reacts to the equation?
What I would first is to find the amount of mols of H3PO4. Since you know that 1 M means there is 1 mol of solution in every 1 liter, you can figure out the moles of the solution. The solution is 6M, so that means that to find the moles of solute in the solution you multiply .750 (750 milliliters converted to liters) by 6. I think you did something similar, but .0075 L makes 7.5 milliliters. This will give you 4.5 mols of H3PO4.Now you can use stoichiometry to find the grams of Ca3(PO4)2. The balanced equation states that it takes 2 mols of H3PO4 to get 1 mol of Ca3(PO4)2:4.5 mol H3PO4 * 1 mol Ca3(PO4)2 / 2 mol H3PO4 = 2.25 mol Ca3(PO4)2Find the molar mass of Ca3(PO4)2 to convert the mols to grams:3*40 + 2*31 + 8*16 = 310 grams / mol2.25 mol Ca3(PO4)2 * 310 grams Ca3(PO4)2 / 1 mol Ca3(PO4)2 = 697.5 grams Ca3(PO4)2You can use the same process to find the mass of water.4.5 mol H3PO4 * 6 mol H2O / 2 mol H3PO4 = 13.5 mol H2O13.5 mol H2O * 18 g H2O / 1 mol H2O = 243 g H2OHope that helped! NB this is not my work just saw it on another website
What is the sequence of events that would occur when acid is added to phosphate buffer.?
There are different variations of phosphate buffer, but if we take the one in which NaH2PO4 is in equilibrium with Na2HPO4, then we can write the following:H2PO4^- H+ + HPO4^2-When and acid (H+) is added, it will react with HPO4^2- to produce H2PO4^-. Since H2PO4 is a weak acid, it will not dissociate appreciable, thus effectively removing the added H+ from solution and maintaining the pH.
What happens when you get an answer like 0 equals 6?
When you get an answer like 0=6 it would be no solution.
Is 5 a solution of 28 equals 80n?
No. If n=5, 80n would be 400, not 28
