Question

3) Find the concentration of Ca2+ and IO-3 in a saturated Ca(IO3)2 solution prepared by adding...

3) Find the concentration of Ca2+ and IO-3 in a saturated Ca(IO3)2 solution prepared by adding Ca(IO3)2 to a 0.015 M solution of KIO3. Ksp of Ca(IO3)¬2(s) is 4.4x10-7M3.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
A saturated solution of Cu(IO3)2 was prepared in 0.015 M KIO3. The copper concentration was found...
A saturated solution of Cu(IO3)2 was prepared in 0.015 M KIO3. The copper concentration was found to be 0.0010 M. Set up an ICE chart and calculate the equilibrium [IO3-] and the Ksp.
a saturated solution cu(io3)2 was prepared in 0.015 m klo3. The copper concentration was found to...
a saturated solution cu(io3)2 was prepared in 0.015 m klo3. The copper concentration was found to be 0.0010 M. Set up an ice table and caunlate the [IO3-] and the Ksp.
Part I: Calculate the concentration of IO3– in a 9.05 mM Pb(NO3)2 solution saturated with Pb(IO3)2....
Part I: Calculate the concentration of IO3– in a 9.05 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 × 10-13. Assume that Pb(IO3)2 is a negligible source of Pb2 compared to Pb(NO3)2. Part II: A different solution contains dissolved NaIO3. What is the concentration of NaIO3 if adding excess Pb(IO3)2(s) produces [Pb2 ] = 3.80 × 10-6 M? Please explain thoroughly. I am SO confused!! Thank you SO much in advance!
Using activities, find the concentration of Ba+2 in a 0.100M (CH3)4N+ IO3- solution saturated with Ba(IO3)2....
Using activities, find the concentration of Ba+2 in a 0.100M (CH3)4N+ IO3- solution saturated with Ba(IO3)2. Assume Ba(IO3)2 makes a negligible contribution to the ionic strength and the Ksp value is 1.5 X 10-9 PLEASE SHOW ALL STEPS!
A group of students conducted a titration of 25.00-mL saturated Ca(OH)2 solution with 0.0480M HCl. The...
A group of students conducted a titration of 25.00-mL saturated Ca(OH)2 solution with 0.0480M HCl. The students found that 10.10-mL of acid was required to reach the equivalence point. Calculate the molar concentration of OH- and Ca2+, the molar solubility, and Ksp of the analyte. Show detailed calculation for each. [OH-] in the analyte: [Ca2+] in the analyte: molar solubility of Ca(OH)2: Ksp of Ca(OH)2:
Perform the following calculations involving concentrations of iodate ions. (a) The iodate ion concentration of a...
Perform the following calculations involving concentrations of iodate ions. (a) The iodate ion concentration of a saturated solution of Ce(IO3)4 was found to be 7.35 ✕ 10−4 mol/L. Find the Ksp. (b) Find the concentration (in M) of iodate ions in a saturated solution of Ca(IO3)2. (Ksp = 6.47 ✕ 10−6)
0.02500 M EDTA solution were used to titrate 10.00 mL saturated Ca(OH)2 solution. EDTA=C10H14N2Na2O8 The average...
0.02500 M EDTA solution were used to titrate 10.00 mL saturated Ca(OH)2 solution. EDTA=C10H14N2Na2O8 The average volume of EDTA solution needed was 11.15 mL to titrate a 10.00 mL saturated solution of Ca(OH)2. milimoles of EDTA= 0.02500(M) *11.15ml = 0.2875milimoles Milimoles of Ca2+= strength * volume = 2.845milimoles ____________________________________________________________ 1.) How many grams of Ca(OH)2 can be dissolved in 1-L solution? 2.) Ksp
Calculate the molar solubility of Ca(IO3)2 in each solution below. The Ksp of calcium iodate is...
Calculate the molar solubility of Ca(IO3)2 in each solution below. The Ksp of calcium iodate is 7.1 × 10−7. (a) 0.070 M Ca(NO3)2 (b) 0.070 M NaIO3
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL)...
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL) = 25.0 mL 2. Concentration of Standardized HCL solution (mol/L) = 0.05 mol/L 3. Buret reading, initial (mL) = 50.0 mL 4. Buret reading, final (mL) = 32.5 mL 5. Volume of HCL added (mL) = 17.5 mL 6. Moles of HCL added (mol) = (concentration of HCl)(Volume of HCl) = (0.05)(19.1) = 0.875 mol. 7.Moles of OH- in saturated solution (mol)=8.75x10^-4 8.the [OH-]...
What is the molar solubility of La(IO3)3 in a 0.830 M solution of Mg(IO3)2? The Ksp...
What is the molar solubility of La(IO3)3 in a 0.830 M solution of Mg(IO3)2? The Ksp for La(IO3)3 = 7.50 10-12
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT