1. Write the charge balance for a MgSO4 and NaNO3 solution that contains Ht, OH, Mg²+, HSO4, SO²-4, MgHSO*4,MgOH+, Na+, and NO 3.A. [SO2-4]+[Mg2+]=[OH-]+[HSO−4]+[H+]+[NO−3]+[MgHSO+4]+[MgOH+]+[Na+]B. [H+]+2[Mg2+]+[MgHSO+4]+[MgOH+]+[Na+]=[OH-]+[HSO-4]+2[SO2-4]+[NO-3]C. [H+]+[Mg2+]+[MgHSO+4]+[MgOH+]+[Na+]=[OH-]+[HSO-4]+[SO2-4]+[NO-3]D. [Mg2+]+[MgHSO+4]+[MgOH+]=[OH-]+[HSO−4]+[SO2−4]+[NO−3] +[H+]+[Na+]2. Select each side of the mass balance equation for an Fe3(PO4)2 solution where the species in solution are Fe2+, PO3-4,HPO42-, H2PO4-, H3PO4, and FeOH+.A. 3([Fe2+]+[FeOH+])=3[PO3-4]+2[HPO2-4]+[H2PO-4]B. 3([Fe2+]+[FeOH+])=[PO3-4]+[HPO2-4]+[H2PO-4]+[H3PO4]C.[Fe2+]+[FeOH+]=2([PO3—4]+[HPO2-4]+[H2PO-4]+[H3PO4])D. 2([Fe2+]+[FeOH+]) = 3([PO3-4]+[HPO2-4]+[H2PO-4]+[H3PO4])3. Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 5.541 using the systematic treatment ofequilibrium. Ksp(Ag2CO3)=8.46x10-12; Ka1(H2CO3)=4.45x10-7; Ka2(H2CO3)=4.69x10-11Use the systematic treatment of equilibrium to solve this problemPlease & Thank you in advance!

“Since you have posted multiple questions, we will provide the solution only to the first question…

1. Write the charge balance for a MgSO4 and NaNO3 solution that contains H+, OH, Mg2+, HSO4, SO²-4, MgHSO*4, MgOH+, Na+, and NO 3. A. [SO2-4]+[Mg2+]=[OH-]+[HSO−4]+[H+]+[NO−3]+[MgHSO+4]+[MgOH+]+[Na+] B. [H+]+2[Mg2+]+[MgHSO+4]+[MgOH+]+[Na+]=[OH-]+[HSO-4]+2[SO2-4]+[NO-3] [H+]+[Mg2+]+[MgHSO+4]+[MgOH+]+[Na+]=[OH-]+[HSO-4]+[SO2-4]+[NO-3] C. D. [Mg2+]+[MgHSO+4]+[MgOH+]=[OH-]+[HSO-4]+[SO2−4]+[NO−3] +[H+]+[Na+]

1. Write the charge balance for a MgSO4 and NaNO3 solution that contains H+, OH, Mg2+, HSO4, SO²-4, MgHSO*4, MgOH+, Na+, and NO 3. A. [SO2-4]+[Mg2+]=[OH-]+[HSO−4]+[H+]+[NO−3]+[MgHSO+4]+[MgOH+]+[Na+] B. [H+]+2[Mg2+]+[MgHSO+4]+[MgOH+]+[Na+]=[OH-]+[HSO-4]+2[SO2-4]+[NO-3] [H+]+[Mg2+]+[MgHSO+4]+[MgOH+]+[Na+]=[OH-]+[HSO-4]+[SO2-4]+[NO-3] C. D. [Mg2+]+[MgHSO+4]+[MgOH+]=[OH-]+[HSO-4]+[SO2−4]+[NO−3] +[H+]+[Na+]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the concentration of Pb2+ in parts per million when 0.069 g of the chloride salt is dissolved in 810.29 mL of water? The density of water is 1.0 g/mL.
Calculate the pH of a solution that is 0.0890 M in a. NaH₂PO4 (K₁1 = 7.11 x 10-³, K 6.32 x 108). pH = b. NaHSO3 (Kat= pH = C. pH= Submit Answer = 1.23 x 10-2, K2= 6.60 x 10-8). H₂NC₂H, NH, CI (K₁1=1.42 x 10-7, K₁2 = 1.18 × 10-10). Try Another Version 8 item attempts remaining
11. Calculate the concentrations of all species present in a 0.416 M H3PO4 solution. Ignore the auto ionization of water. Kat = 7.5 x 10-3, Kaz = 6.2 x 10-8, Ka3 = 4.8 x 10-13,
Calculate the pH of the following solutions:1- 0.01 M NaHS2- 0.005 M NaH PO,3- 0.005 M NaHPO4- 0.005 M Na PO 5- 0.1 M NH,CN
8. Calculate the pH of a solution with [H3O']= 9 × 101 M.
Calculate the concentration of free Ca²⁺ in a solution of 0.10 M CaY²⁻ at pH 10.00. (K= 5.0 × 10¹⁰) 2.4 × 10⁻⁶ M5.6 × 10⁻¹² M 5.6 x 10⁻¹¹ M 7.2 × 10⁻¹³ M None of the given.
ASK YOUR TEAC The hydronium ion concentration in a sample of springwater is found to be 6.3x10 M at 15°C. What is the concentration (in M) of hydroxide ions in the springwater? (K = 4.57x 10¬15 at this temperature.) 40 t. Supporting Materials EPeriodic Table Constants and Supplemental Data Factors Additional Materials Section 14.2 MacBook Air 吕0 888 DII DD F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 F12 %23 $ & 1 2 4 7 8. Q W E Y { A G K C V B N T F. R D. #3 Σ
How do you explain the pattern/trend in the distance between the anion of an acid and H3O+? The acid strength is HCl > HNO3 > HF > HOCl, but I don't understand why the lengths vary like this. Or does it have to do with electronegativity? If it does have to do with electronegativity, why doesn't HF have the shortest length? Or is it because OCl- is more elctronegatvie than F-? Also, does an acid's strength decrease/increase with increasing electronegativity of its conjugate base? When looking at the trend, HI is stronger than HBr, which is stronger than HCl. However, HClO4 is stronger than all of these acids, which I don't understand why.
not graded, just a practice I want to learn how to do.
Ind the solution is acidic. The pH is less than 7 and the solution is basic. ion 9 Which ONE of the following pairs reacts in a 1:1 ratio during a neutralization reaction? Selected Answer. H3PO4 + KOH Answers HCIO4 + Са(ОН)2 H2SO4 + Ba(OH)2 H3PO4 + KOH H2SO4 + AI(OH)3 H3PO4 Ca(OH)2 estion 10 Besides water what else is produced during the neutralization reaction shown below:
1. What is the pH of ammonia if the [H3O+] of ammonia is 3.7 x 10-11 M? Use 2 decimal places for pH. 2. A patient with respiratory alkalosis has a blood plasma pH of 7.22. What is the [H3O+] of the blood plasma? Use 2 significant figures for concentration. 3. Calculate the pH of a solution with a [OH-] concentration of 3.0 x 10-5 M. Use 2 decimal places for pH.
Which of the following is the correct net ionic equation for the reaction shown below? 2 HNO3 (aq) + Ca(OH)2 (aq) --> Ca(NO3)2 (aq) + 2 H2O (l) a. Ca(OH)2 (aq) --> Ca2+ (aq) + 2 OH- (aq) b. Ca2+ (aq) + 2 NO3- (aq) --> Ca(NO3)2 (aq) c. 2 H+ (aq) + OH- (aq) --> 2 H2O (l) d. H (aq) + OH (aq) --> H2O (l) e. none of the above