[ОН ] pH pH pH Calculated раper meter pH 1. 0.1 M 2. 0.01 M 3. 0.001 M 4. 0.0001 M [H,O° ] pH pH Calculated раper meter pH 5. О.1 М 6. 0.01 M 7. 0.001 M 8. 0.0001 M
Q: Determine the pOH of a solution that is 0.110 M in CO3?-. For carbonic acid (H2CO3), Kal = 4.3 x…
A: B.) CO32- is a second conjugate base of H2CO3. So to calculate it's pOH , we would need its Kb1 ,…
Q: A solution is made from 0.51 M NH3 and 0.48 M NH4Cl. What is the pH if the Kb for NH3 is 1.8x10-5?…
A:
Q: What is the pH of a 0.0015 M solution of HBr? 5.65 You need the Ka value to answer this…
A: What is the pH of a 0.0015 M solution of HBr?
Q: Calculate the pH for an aqueous solution of pyridine that contains 4.15 x 10^-4 hydroxide ion. Group…
A: Given, [OH-] = 4.15×10-4 M pOH = -log[OH-] pOH = -log[4.15×10-4 ] pOH = 3.38
Q: Calculate the pH for an aqueous hydroiodic acid solution that contains 3.15 x 10^-3 hydronium ion.…
A: pH is the negative logarithm of Hydrogen ion (hydronium ion) concentration. It stands for power of…
Q: Find the pH and the pOH of the solution 1. A 0.000469 M solution of sodium hydroxide 2. A…
A: Given that [NaOH] = 0.000469 M [H2SO4] = 0.000896 M We know that pH = – log[H+] pOH = – log[OH–] pH…
Q: Calculate the [H+] in a solution that has a pH of 12.01. 9.8 × 10-13 M 12.0 M 2.0 M 1.0 × 10-2 M…
A: Given PH = 12.01 -log[H+] = 12.01 log[H+] = -12.01 [H+] =…
Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=3.9×10−5…
A:
Q: Determine the pH of 5.416 x 10-8 M of HCl. (use the systematic treatment) Determine the pH of 7.814…
A: 1) Concentration of HCl solution = [HCl] = 5.416 x 10-8 M pH of the solution = ? Note: HCl is a…
Q: What is the pH of 10.0 mL of 0.0020 M HCl? 3.70 10.0 5.70 2.70 0.70
A: Given the on concentration of HCl solution = 0.0020 M The pH of 10.0 mL of 0.0020 M HCl =
Q: What is the [H3O+] in a solution with a pH of 8.66? Group of answer choices 2.2 × 10-9 M 1.5 × 10-5…
A:
Q: The Ka value for acetic acid, CH3COOH(aq), is 1.8×10 −5. Calculate the pH of a 1.40M acetic acid…
A: Acetic acid dissociate in aqueous solution as: CH3COOH→CH3COO-+H+
Q: Calculate the pH of 0.048 M HNO2 solution (Ka = 4.5 x 10-4) . HNO2 (aq) --> H+ (aq) +NO2-(aq)
A: Given Concentration of HNO2 = 0.048 M Ka = 4.5 × 10-4
Q: Consider a solution where 1.00 grams of PrCl3 (praseodymium (III) chloride) is dissolved in enough…
A: Given, Mass of PrCl3 = 1.00 g Volume in mL = 50.00 mL a). Calculate the pH of the solution. b).…
Q: What is pH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10…
A: 1.05 M NH3 and 0.98 M NH4NO3 The NH4NO3 dissociate as ; NH4NO3 = NH4+ + NO3- So the Concentration…
Q: A chemist dissolves 417. mg of pure potassium hydroxide in enough water to make up 160. mL of…
A: Applying concept of molarity and PH and POH. POH= -log [OH-]
Q: Calculate the pH for each H+H+ concentration. [H+]=1×10−7 MpH=[H+]=1×10−7 M [H+]=0.01…
A: All acidic solutions possess a specified pH value which tends to denote the amount of H+ ions…
Q: Which solution will have the lowest pH? 0.10 M HCN 0.10 M H2CO3 0.10 M NaCl 0.10 M HNO3 0.10 M…
A: The given data: The concentration of HCN = 0.10 M The concentration of H2CO3 = 0.10 M The…
Q: The pH of a human blood sample is 7.30. What is concentration of OH- in blood? a. 5.01 ×× 10-8 M…
A:
Q: What is the concentration of a hydrosulfuric acid solution with a pH of 2.34? Group of answer…
A:
Q: Determine both the H and the pH in a 0.0541 M solution of HNO3 at 25 °C? H= Type your answer here…
A: The concentration of HNO3 solution = 0.0541 M HNO3 → H+ + NO3− The concentration of H+, [H+] =…
Q: Find the ph of a solution 1.8 M in KCl. Report answer to two decimal places
A: PH of solution = ? Concentration = 1.8 M
Q: Calculate the pH of 0.200 M HNO3(aq). 1.609 -1.140 0.699 2.000 13.800
A:
Q: What is the pH of a solution containing 0.1279 M HOCN and 0.1517 M KOCN? Ka = 3.50e-4. 10.544…
A: Acid, [HOCN] = 0.1279 M Salt, [KOCN] = 0.1517 M Ka = 3.50 × 10-4
Q: Find the pH of the following acidic solutions: A 0.001 M solution of HCl (hydrochloric acid). 3…
A: 'As you have posted multipart question, we will solve first three. If you want any specific part to…
Q: 1a) Determine the pH of 0.035 M NaF (pKa = 3.1). 1b) Determine the pH of 0.055 M oxalic acid…
A: It's a multiple part question. Given information, 1 (a) [NaF] = 0.035 M pKa = 3.1 1 (b) [oxalic…
Q: Calculate the pH of a formic acid solution that contains 1.42% formic acid by mass. (Assume a…
A: Molarity of formic acid, C = moles of solutevolume of solution = 1.42 x 1.01 x 100046 x 100 = 0.312…
Q: A beaker contains a solution with 0.70 moles of HNO3. 0.60 moles of KOH is added. The final volume…
A:
Q: An aqueous solution at 25.0°C contains [H+] = 0.099 M. What is the pH of the solution? Group of…
A: We have given that the concentration of [H+] = 0.099 M we know the formula to calculate the pH of…
Q: OH + HSO, H2O + SO, 2. Convert each H3O concentration to a pH value. a. 1x10 M b. 1x 10" M c.…
A: Question 2) pH pH can be define as negative logarithm of H+ or H3O+ ion concentration. pH =…
Q: Solution 1 has [H+] = 9.7×10-7 M, and solution 2 has [H+] = 1.4×10-4 M. Calculate pH of both…
A:
Q: What is the concentration of an aqueous HI solution that has a pH of 2.26? 1.82 x 10-2 M…
A: Given that, pH = 2.26 Then, [HI] = ?
Q: All of the following statements about the pH scale are true EXCEPT Group of answer choices: Blood is…
A: Using the relation of pH and [H3O+] , concentration of hydronium ion, [H3O+] can be determined.
Q: A 0.250 M solution of a weak base has a pH of 9.91. Calculate the Kb of this base. Kb = ______ x…
A:
Q: What is the pH of a solution with a hydronium ion concentration of 3.9x10-7 Record to the tenth's…
A:
Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 10.49. Calculate the…
A: pH is equal to the negative logarithm of hydrogen ions
Q: Which of the following has the lowest pH? 3.9x10-3 M HPO42- (Ka3=4.2x10-13) 0.00010 M H3BO3…
A:
Q: In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of…
A: In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of…
Q: What is the pH of a 4.514.51 ×10−2×10-2 M solution of KOH? 1.351.35 11.511.5 6.956.95 12.712.7…
A: pH :- The negative logarithm to the base 10 of H+ ion concentration expressed in mol/L of a…
Q: Calculate the pH for each H3O+ concentration. [H3O+] = 1×10−7 M pH= [H3O+] = 0.001 M pH=…
A: Answer:- This question is answered by using the simple concept of calculation of pH using the…
Q: Calculate pH if [OH ] = 2.0 x 10-3 M.
A: We have to Calculate the PH of the given (OH-) concentration
Q: What is the pH of a solution of 0.65 M Acetic Acid? Select an answer and submit. For keyboard…
A:
Q: Kw = 0.114 x 10-14 at 0°C = 1.00 x 10-14 at 25°C Kw Kw = 2.42 x 10-14 at 37°C Kw = 9.61 x 10-14 at…
A:
Q: Water has a pH of 7. If 0.1 mL (about one drop) of 1.0 M HNO3 is added to 100 mL of water, the…
A: Given, Concentration of HNO3 = 0.001 M Initial pH of water = 7 The property of logarithmic that…
Q: Write the acid concentration or the pH for each of the following instances: A.) a 0.5 M solution…
A: A.) a 0.5 M solution H2SO4:
Q: Chemistry Calculate the pH of 0.0035 M KOH. Note: You are starting with a base. 11.54 7.00 13.99…
A:
Q: Calculate the OH– concentration & pH of a 0.45 M NH3 solution (Kb=1.75 × 10–5)
A: NH3 is a weak base Given dissociation constant of NH3 is (Kb) =1.75×10-5 Concentration of NH3 is =…
Q: What is the pH of a 0.0253 M solution of NaOBr? (For HOBr, Ka = 2.5 × 10−9) Enter your answer using…
A:
Q: Determine both the H and the pH in a 0.0541 M solution of HNO3 at 25 °C? [H*]= H= Type your answer…
A:
Q: What is the pH of 0.1510 M selenious acid solution, H2SeO3? H2SeO3(aq) + H2O(l) → HSeO3−(aq) +…
A: As the second ionization constant Ka2 is very less than first ionization constant Ka1, the Ka2 can…
I just need the calculated PH
![[ОН ]
pH
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О.1 М
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0.01 M
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0.001 M
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- Please answer fast it’s very important and urgent I say very urgent so please answer super super fast please For the image attached For 1. a Mass of metal: Trial 1 is 35.0228 g Trial 2 is 35.0915 g Trial 3 is 34.0821 g Mass of water: Trial 1 is 20.0177 g Trial 2 is 20.0250 g Trial 3 is 20.0168 g For delta t of water: Trial 1 is 15.5 C Trial 2 is 15.7 C Trial 3 is 15.1 C For delta t of metal Trial 1 is 80.1 C Trial 2 is 80.2 C Trial 3 is 79.5 C For B my calculated Specific heat is: Trial 1 is 0.462 Trial 2 is 0.467 Trial 3 is 0.466Help with questions 2-3 on work sheet using data pleaseQNO1. BEER'S LAW DEFINITION INTRODUCTION AND FULL DERIVATION NEED. DERIVE STEPS BY STEPS WITH CALCULATION OK THANKS . Only Human expert solve no AI
- Liquid silver's chemical name is: a. Ag (only) b. Si (liquid) c. Ag (liquid) d. Hg (liquid) I need explanation in a research way. Please don't base the answer to any articles that can be seen in google instead base it with a research paper or any studies with authors. Book-supported is also okay.Provide the remaining data missingNH4+ {aq) + NO2(aq) -> N2(g) +2H2O{l} Data Initial [NH4+] Initial [NO2-] rate 1 0.0100 0.200 5.4 x10-7 2 0.0200 0.200 10.8x10-7 3 0.0400 0.200 21.5x10-7 4 0.200 0.0202 10.8x10-7 5 0.200 0.0404 21.6x10-7 6 0.200 0.0808 43.3x10-7 Find x,y,k
- Consider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2] [I–] [H+] rate I 0.100 M 5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec The rate law for this reaction isConsider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2] [I–] [H+] rate I 0.100 M 5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec The rate law for this reaction is a. rate = k[H2O2][I–][H+] b. rate = k[H2O2][H+] c. rate = k[H2O2]2[I–]2[H+]2 d. None of these e. rate = k[H2O2][I–] f. rate = k[I–][H+]Consider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2] [I–] [H+] rate I 0.100 M 5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec The rate law for this reaction is a. rate = k[H2O2]2[I–]2[H+]2b. rate = k[I–]c. None of thesed. rate = k[I–][H+]e. rate = k[H2O2][I–][H+]f. rate = k[H2O2][H+]
- Consider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2][I–][H+]rate I 0.100 M 5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec a. The rate law for this reaction is a. rate = k[H2O2][I–][H+] b. rate = k[H2O2]2[I–]2[H+]2 c. rate = k[I–][H+] d. rate = k[H2O2][H+] e. rate = k[H2O2][I–]In aqueous solution, chlorine dioxide oxidizes iodide ion to iodine and chlorine dioxide is reduced to chlorite ion. 2ClO2 (aq) + 2 I- (aq) ----> 2ClO2- (aq) + I2 (aq) The concentration in molarity, of ClO2 was measured at various time points. The data was plotted and the plot of [1/[ClO2] versus time in seconds was most linear. The linear regression equation for the plot is y= 7.60x10-2 (t) + 2.353. What is the concentration of ClO2 at 2.00 minutes if the initial concentration of ClO4 ia 0.425 M? a.) 0.0872 M b.) 2.50 M c.) 11.5 M d.) 0.399 MPls solve this problem and I upvote. Do not reject if it's hard for you skip it so one of the expert can do it. Thank you. I pray for your wellbeing