Question

Solid calcium hudoxide reacts with phosphoric acid according to the following equation: 3 Ca(OH)2+ 2H3PO4--- Ca3(PO4)2+...

Solid calcium hudoxide reacts with phosphoric acid according to the following equation:

3 Ca(OH)2+ 2H3PO4--- Ca3(PO4)2+ 6 H2O

what in volume of 0.0220 M phosphoric acid can be neutralized by 94.651 grams of Calcium hydroxide

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

IF:

3moL Ca(OH)2 + 2moL H3PO4 ---> 1moL Ca3(PO4)2 + 6moL H2O

3moLx74 g/moL Ca(OH)2 + 2moLx98g/moL H3PO4 ---> 1moLx310g/moL Ca3(PO4)2 + 6moLx18g/moL H2O

222 g Ca(OH)2 + 196 g H3PO4 ---> 310 g Ca3(PO4)2 + 108 g H2O

AND IF:

222g of pure Ca(OH)2 can be neutralized 196g of pure H3PO4

THEN:

How much pure phosphoric acid can be neutralized by 94.651g pure Calcium hydroxide?

94.651g Ca(OH)2 x (196g H3PO4/222g Ca(OH)2) = 83.565g of pure H3PO4

How much 0.0220M phosphoric acid solution can be obteined wich 83.565g of pure H3PO4?

[M]= Mass/(FwxV)

V= Mass/(Fwx[M])

V= 83.565g H3PO4/(98g/moLx0.0220 moL/L)

V= 83.565g H3PO4/(98g/moLx0.0220 moL/L)

V= 38.76 L H3PO4 solution.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
2 H3PO4(aq) + 3Ca(OH)2(aq) = Ca3(PO4)2 (s) + 6 H2O(l) 1. a.Calculate the volume of .0500...
2 H3PO4(aq) + 3Ca(OH)2(aq) = Ca3(PO4)2 (s) + 6 H2O(l) 1. a.Calculate the volume of .0500 M phosporic acid that would be required to exactly react with 20.0 ml of 0.100 M calcium Hydroxide b. What mass of calcium phosphate will precipitate?
Consider the following balanced equation: 2H3PO4(aq) + 3Ca(OH)2(s) → 6H2O(l) + Ca3(PO4)2(s) If 13.6 moles of...
Consider the following balanced equation: 2H3PO4(aq) + 3Ca(OH)2(s) → 6H2O(l) + Ca3(PO4)2(s) If 13.6 moles of H3PO4(aq) and 35.3 moles of Ca(OH)2(s) are allowed to react, and the percent yield is 84.5%, how many moles of H2O(l) will actually be produced? 60.5 moles 87.2 moles 95.2 moles 76.7 moles 34.5 moles
Using the following equation K3PO4(aq)+Ca(NO3)2(aq)---Ca3(PO4)2(s)+KNO3(aq) If you start with 4.6 grams of CA(NO3)2 and a stoichiometric...
Using the following equation K3PO4(aq)+Ca(NO3)2(aq)---Ca3(PO4)2(s)+KNO3(aq) If you start with 4.6 grams of CA(NO3)2 and a stoichiometric quantity of K3PO4 and produce a 92% yield CA3(PO4)2, what is the actual yield in grams
Phosphorus occurs naturally in the form of fluorapatite, CaF2·3 Ca3(PO4)2, the dot indicating 1 part CaF2...
Phosphorus occurs naturally in the form of fluorapatite, CaF2·3 Ca3(PO4)2, the dot indicating 1 part CaF2 to 3 parts Ca3(PO4)2. This mineral is reacted with an aqueous solution of sulfuric acid in the preparation of a fertilizer. The products are phosphoric acid, hydrogen fluoride, and gypsum, CaSO4·2 H2O. Balance the chemical equation describing this process. (Type your answer using the format CO2 for CO2.) CaF2·3 Ca3(PO4)2(s) + (aq) + (l) (aq) + HF(aq) + CaSO4·2 H2O(s)
Using the following equation K3PO4(aq)+Ca(NO3)2(aq)---Ca3(PO4)2(s)+KNO3(aq) Complete balanced equation and answer If you start with 3.2g of...
Using the following equation K3PO4(aq)+Ca(NO3)2(aq)---Ca3(PO4)2(s)+KNO3(aq) Complete balanced equation and answer If you start with 3.2g of K3PO4, how many grams of CA(NO3)2 are needed to reach stoichiometric quantities?
Solid calcium bicarbonate (Ca(HCO3)2) reacts with aqueous hydrochloric acid (HCl) to form aqueous calcium chloride, liquid...
Solid calcium bicarbonate (Ca(HCO3)2) reacts with aqueous hydrochloric acid (HCl) to form aqueous calcium chloride, liquid water, and carbon dioxide gas. (a) Write the balanced molecular equation, complete ionic equation, and net ionic equation for the process. [Hint: Don’t forget the physical states of the reactants and products.] Balanced Molecular Equation: Complete Ionic Equation: Net Ionic Equation: (b) A CHEM 104 student is trying to carry out this reaction in the laboratory. What is the minimum amount of 0.2102 M...
1. Show the calculation of the mass of Ca3(PO4)2 needed to make 200 ml of a...
1. Show the calculation of the mass of Ca3(PO4)2 needed to make 200 ml of a 0.128 M solution. 2. Show the calculation of the volume of 0.987 M solution which can be prepared using 24.6 grams of NaNO3. 3. Show the calculation of the volume of 0.238 M solution which can be prepared using 13.4 grams of Ca3(PO4)2.
The commercial production of phosphoric acid, H3PO4, can be represented by the equation 1540 g 282...
The commercial production of phosphoric acid, H3PO4, can be represented by the equation 1540 g 282 g 317 g 1090 g 282 g Ca3(PO4)2 + 3SiO2 + 5C + 5O2 + 3H2O → 3CaSiO3 + 5CO2 + 2H3PO4 310 g/mol 60.1 g/mol 12.0 g/mol 32.0 g/mol 18.0 g/mol The molar mass for each reactant is shown below the reactant, and the mass of each reactant for this problem is given above. Which substance is the limiting reactant? The commercial production...
How many grams of Ca3(PO4)2 precipitate can form by reacting 169.1 mL of 1.9 M CaBr2...
How many grams of Ca3(PO4)2 precipitate can form by reacting 169.1 mL of 1.9 M CaBr2 with an excess amount of Li3PO4, given the balanced equation: 2 Li3PO4 (aq) + 3 CaBr2 (aq) --> 6 LiBr2 (aq) + Ca3(PO4)2 (s)
The hydroxide ion concentration, [OH-], in each of your trials can be calculated from the concentration...
The hydroxide ion concentration, [OH-], in each of your trials can be calculated from the concentration of the hydrochloric acid, 0.050 M HCl, and the volume of both the HCl and Ca(OH)2 used in the titration. According to the net ionic equation (calcium hydroxide, Ca(OH)2 (s), in water) determine the ratio of moles of calcium ion, Ca2+, to moles of hydroxide ion, OH-, in the solution of calcium hydroxide, Ca(OH)2. Using this ratio, determine the molarity of calcium ion in...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT